Problem 7.1. Determine the molecular formula of a monochloroalkane containing 38.38% chlorine. Give graphic formulas and names of all compounds that correspond to this formula.
Solution:
M(R + R 1) = 60 - 12 - 32 = 16 g / mol, therefore, only the H atom and methyl CH 3 can be radicals.
Ester formula HCOOCH 3
Problem 7.8. Upon combustion of 9 g of primary amine, 2.24 liters of nitrogen (n.o.) were released. Determine the molecular formula of the amine and name it.
Solution:
1. Stoichiometric scheme of the amine combustion reaction:
2. Determine the amount of amine substance and its molar mass:
n(RNH 2) = 1 / 2n(N 2) = 2.24 / 22.42 = 0.05 mol
M(RNH 2) = 9 / 0.05 = 45g / mol
3. Find the molar mass of the radical:
M(R) + 14 + 2 = 45 M(R) = 29g/mol
Amine formula C 2 H 5 NH 2
Problem 7.9. Establish the molecular formula of a saturated diatomic alcohol containing 57.69% carbon.
Solution:
1. General formula of saturated dihydric alcohol C n H 2 n (OH) 2
2. ω(C) = 12n / 12n + 2n + 34 = 0.5769 n = 5 C 5 H 10 (OH) 2
Problem 7.10. During the combustion of an organic oxygen-free compound, 4.48 liters (n.s.) of carbon dioxide, 3.6 g of water and 2 g of hydrogen fluoride were released. Determine the molecular formula of an organic compound.
Solution:
1. n(CO 2) = 4.48 / 22.4 = 0.2
n(H 2 O) = 3.6 / 18 = 0.2
Option 7
1. The Kucherov reaction is widely used to obtain acetaldehyde in
factory scale. How much of this aldehyde can be obtained from
100 kg of technical calcium containing 20% impurities, if the yield
aldehyde is 80?
2. What amount of iodoform can be obtained from 200 kg of acetone?
Write the reaction equation.
3. The mass fractions of carbon, hydrogen and oxygen in the aldehyde are
respectively 62.1%, 10.3% and 27.6%. How much hydrogen will be required?
for the hydrogenation of this aldehyde weighing 14.5 g to alcohol? Volume
calculate under normal conditions.
4. During the oxidation of some oxygen-containing organic substance
weighing 1.8 g with an ammonia solution of silver oxide, we obtained silver weighing
5.4 g. Which organic substance is subject to oxidation?
Option 8
1. Mass fraction of the yield of the reaction product during the oxidation of ethanol by volume
120 ml (ρ = 0.8) is 90%. Calculate the mass, amount of substance and
number of aldehyde molecules formed.
2. What amount of acetone will be obtained from 1 ton of calcium acetate?
3. What volume of formaldehyde must be dissolved in water weighing 300 g for
obtaining formaldehyde with a formaldehyde mass fraction of 40%? Volume
calculate under normal conditions. What mass of formalin will be
received?
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4. When ethanol weighing 13.8 g interacts with copper (II) oxide weighing 28 g
obtained an aldehyde whose mass was 9.24 g. Determine the yield
reaction product.
Option 9
1. What volume of air and what mass of methyl alcohol was needed for
obtaining formalin weighing 4 tons with a mass fraction of formaldehyde 40% at
oxidation of methyl alcohol?
2. What mass of limestone needs to be burned in order to use the carbide method?
obtain acetylene, which would be enough to synthesize a solution of acetaldehyde
weighing 1800 kg with a mass fraction of 25%?
3. Upon interaction of saturated aldehyde weighing 5.8 g with excess
Copper (II) hydroxide upon heating formed 14.4 g of copper oxide precipitate
(I). Determine the molecular formula of the aldehyde.
4. During the oxidation of ethanol, an aldehyde was formed with 80% yield. At
interaction of the same mass of ethanol with metallic sodium was released
hydrogen, which occupies 2.8 liters under normal conditions (yield
quantitative). Determine the mass of the aldehyde formed in the first
reactions.
Option 10
1. The oxidation of ethanal released 2.7 g of silver. Calculate how much
liters of acetylene were required to obtain the required mass of ethanal
(Well.)?
2. From n-butyl alcohol by a three-step synthesis, obtained
methyl ethyl ketone. How much ketone can be obtained from 0.74 kg
starting alcohol, if the yield of reaction products at each stage is
is 50%?
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3. For the quantitative oxidation of 4.6 g of an equimolecular mixture of two
monohydric alcohols into aldehydes required 7.96 g of copper (II) oxide.
Determine the structure of the starting alcohols if, upon interaction
the resulting mixture of aldehydes with an ammonia solution of silver oxide
32.4 g of sediment was released.
4. From calcium carbide weighing 7.5 g, containing impurities (mass fraction
impurities is 4%), we obtained acetylene, which was converted into aldehyde
according to Kucherov's reaction. What mass of silver will be released during the interaction
of the total aldehyde obtained with an ammonia solution of silver oxide?
Option 11
1. An effective method for the synthesis of acetaldehyde is direct
oxidation of ethylene in the presence of palladium chloride. What volume of ethylene
is consumed to produce an aldehyde weighing 352 kg, if the mass fraction
is the aldehyde yield 95% of theoretical?
2. When a portion of ethanol interacts with sodium, 7.84 liters (no.) of gas are collected.
Find the mass of aldehyde formed during the oxidation of the same portion
alcohol, if the practical yield in the second reaction is 72.6%.
3. Some organic compound A is a product of treatment with water
compound B (mass composition: 37.7% C, 6.3% H, the rest Cl; 12.7 g
compounds in the vapor state occupy a volume of 2.24 liters at N. y.) - at
reduction with hydrogen goes into secondary alcohol B. Remove
chemical formulas of compounds A, B, C, name them.
4. When oxidizing 100 g of a solution of formaldehyde and ethanol in water
potassium permanganate, 30 g of carboxylic acid and gas were formed, which
when passed into an excess of barite water, it gives 20 g of sediment. Define
mass fraction of formaldehyde and alcohol in the original solution.
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Option 12
1. How much 58% aqueous solution of acetone can be obtained by oxidation of 1 t
secondary propyl alcohol (excluding losses)? Write the equation
reactions.
2. When pentane-3 reacts with hydrazine, hydrazone is formed. How many
take ketone to obtain 30 kg of product, if its yield is 70% of
theoretical?
3. An equivalent mixture of acetylene and formaldehyde reacts completely with
69.6 g Ag2O dissolved in ammonia. Determine the composition of the initial mixture.
4. How much formaldehyde is contained in the solution?
volume 3 l and density 1.06 g/ml, the mass fraction of CH2O in which is equal to
20%?
Option 13
1. Acetone is used in industry as a solvent
paint and varnish materials. What mass of propanol-2 is consumed for
obtaining acetone with a volume of 700 l (ρ = 0.793), if the mass fraction of the yield
acetone is 89% of theoretical?
2. A mixture weighing 21 g (82.9% aldehyde, the rest alcohol) reacts completely
with 69.6 g of silver(I) oxide in ammonia solution. Set titles
components of a mixture if their molecules contain the same number of atoms
carbon and alcohol can be obtained from an aldehyde (and vice versa).
3. Formaldehyde obtained from the dehydrogenation of methanol was dissolved in
water and received 100 g of solution with a mass fraction of 9%. What is the mass of methanol
has it been used up?
4. What mass of solution with a mass fraction of acetaldehyde of 20% is formed,
if the aldehyde was obtained with a yield of 75% from acetylene with a volume of 6.72 l (no.)
by Kucherov's reaction?
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Option 14
1. How many grams of isopropyl alcohol will be required to obtain
by oxidizing 87 g of ketone, if its yield is 90% of
theoretical?
2. During catalytic hydrogenation of 26 g of a mixture of methanal and ethanal
16.8 liters (no.) of gas are consumed. Establish the molar composition of the initial mixture.
3. A certain ketone weighing 1.856 g in the form of steam at 27ºC and a pressure of 740 mm
rt. Art. occupies a volume of 0.809 liters. Determine the relative molecular
the mass of the ketone, derive its form and name the ketone.
4. A mixture of gases formed during the thermal decomposition of 33.6 g of methane,
passed into an excess of ammonia solution Ag2O, while the volume of the mixture
gases decreased by 20%. What volume of methane was converted into acetylene?
What mass of acetaldehyde could be obtained from the resulting
acetylene, if the yield in the Kucherov reaction is 70%?
3. Carboxylic acids and esters
Option 1
1. Establish the molecular formula of the limiting monobasic carbonic acid
acid, the sodium salt of which contains 37.5% carbon.
2. Methanol, what mass, can enter into an esterification reaction with 50 g
84% acetic acid solution?
3. What amount of acid and alcohol is required to obtain 150 g
isovalerian isoamyl ether (apple essence), if the yield
is 80% of the theoretical?
4. Calculate the mass of glycerin obtained from the hydrolysis of 1 t
technical fat formed by glycerin and stearic acid,
if the purity of the fat is 89% (by weight), and the practical yield
product is 76%.
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Option 2
1. What is the mass of 20% formic acid solution required for
neutralization of 0.1 mol sodium hydroxide?
2. What is the mass of acetic acid required to obtain 2 mol
methyl acetate, if the yield of ether from the theoretically possible is
50%?
3. An aqueous 0.1 M solution of monochloroacetic acid has a pH = 2.92.
Determine the degree of dissociation (in%) of the acid.
4. For complete neutralization of 9.62 g of a mixture of acetic and formic acids and
acetaldehyde consumed 42.68 ml of 16% potassium hydroxide solution
with a density of 1.148 g/ml. When treating the initial mixture with ammonia
a solution of silver (I) oxide formed a precipitate; for complete transfer into solution
of this precipitate 48 g of 63% nitric acid were used. Determine mass composition
(in%) of the initial mixture of acids and aldehyde.
Option 3
1. What volume of methane will be required to synthesize 30 kg of formic acid
by oxidation, with a product yield of 50% (n. y)?
2. What is the mass fraction of the dissolved substance in the solution obtained by
dissolving 40 g of sodium acetate in 200 g of water?
3. Establish the molecular formula of saturated carboxylic acid,
the sodium salt of which contains 33.82% metal.
4. There are 96% aqueous solution of ethyl alcohol and 85% solution of acetic acid
acids. Determine the masses (in grams) of these solutions required for
synthesis of 35.2 g of ester (practical yield 80%).
Option 4
1. How much acetic acid is required to obtain 118.8 g of ethyl acetate
at 90% of its output?
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2. Establish the formula of saturated carboxylic acid, methyl ester
which contains 9.09% hydrogen.
3. When ethylene interacts with carbon monoxide and water at 300 - 400ºС and
100 atm in the presence of a catalyst, acid is formed. What volume
ethylene will be required to obtain 1 ton of propionic acid using this method
acid?
4. To obtain benzoic acid, 32.4 g of benzyl alcohol was oxidized.
The oxidizing agent was not enough, so a mixture of products was formed
oxidation. For analysis, the resulting mixture was first treated with excess
NaHCO3, which released 4.48 l of CO2, and then an excess of ammonia
Ag2O solution, and 10.8 g of precipitate was formed. Define mass
proportion of oxidation products in the mixture.
Option 5
1. How many liters of natural gas (N.G.) will be required to produce 64.4 kg
formic acid by catalytic oxidation of methane? In natural
gas contains 98% methane by volume.
2. Made from technical calcium carbide (74% purity by weight)
acetic acid was synthesized, 200 ml was used to neutralize it
5.5 M potassium hydroxide solution (solution density 1.2 g/ml). What mass
(in grams) of technical reagent consumed?
3. 1 liter of 0.05 M aqueous solution of monochloroacetic acid contains
0.002 g of hydrogen cation. Calculate the degree of dissociation (in%) of the acid.
4. With complete oxidation of 3.84 g of organic compound, 2.24 l are obtained
(n.a.) carbon dioxide, 1.8 ml of water and 0.02 mol of sodium carbonate. What are
formula and name of the compound?
Option 6
1. When a 20% solution of acetic acid weighing 120 g interacts with
An ester was formed with methyl alcohol. What is the mass of methanol
reacted?
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2. A 5 g portion of magnesium was treated with 105 ml of 10% formic acid
(solution density 1.03 g/ml). Find: the volume (no.) of the gas released,
mass fraction of salt in the filtered product (after the end of the reaction)
clear solution.
3. For hydrogenation (at the double bond) of a portion of oleic acid,
obtained by saponification of fat, 14.56 m3 consumed
(n.a.) gas. Calculate
the mass of the fat taken, if it contains 8% inert impurities.
4. By bromination of СnН2n+2 we obtained 9.5 g of monobromide, which, when
treatment with a dilute NaOH solution turned into
oxygen-containing compound. Its vapors with air are passed over
hot copper mesh. When processing the resulting
new gaseous substance with an excess of ammonia solution Ag2O
43.2 g of sediment was released. What hydrocarbon was taken and in what quantity,
if the yield at the bromination stage is 50%, the remaining reactions proceed
quantitatively.
Option 7
1. How much bicarbonate of soda is needed to neutralize 50 g 30%
formic acid solution?
2. A 20 g portion of a metal mixture containing 40% copper (by weight,
the rest is magnesium), treated with excess acetic acid. Define
mass fraction (in%) of salt in the final solution, after filtration
whose mass turned out to be 355 g.
3. Three-stage synthesis of 33 l of ethyl acetate (density 0.8 kg/l) from ethylene
proceeded with a practical yield of 50% (stage I), 80% (stage II) and 75% (stage III
stage). Find the consumed volume (n.v.) of the starting alkene.
4. To obtain acetic acid, the starting material was
Technical calcium carbide containing 4% impurities was used. Which
the mass of CaC2 was consumed if the neutralization of the resulting
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acetic acid required 224 g of 20% KOH solution? (Reaction
Kucherova proceeds with a yield of 80%).
Option 8
1. How much hydrogen (n.u.) can be obtained from 30 g of acetic acid and 24 g
magnesium, if it is known that 20% of hydrogen is lost?
2. Formic acid is decomposed by concentrated sulfuric acid into
carbon monoxide and water, and oxalic acid in similar conditions - to carbon dioxide and
carbon dioxide and water. From a certain mixture of these acids we obtained 0.672 l
(n.u.) a mixture of carbon oxides, which was passed through lime water.
1 g of sediment fell. Set the mass fraction (in%) of oxalic acid in
mixtures of acids.
3. For complete saponification, 22.2 g of monobasic carboxylic ester
acid, a 10% sodium hydroxide solution with a density of 1.1 g/ml was consumed and
volume 136.5 ml (taken with 25% excess). Specify the reagent ether (two
possible options).
4. 26.8 g of a mixture of two monobasic carboxylic acids was dissolved in water.
Half of the solution was treated with an excess of ammonia oxide solution
silver, and 21.6 g of silver was released. To neutralize the entire mixture
acids required 0.4 mol NaOH. Determine structural formulas
acids and their amounts in the mixture (in grams).
Option 9
1. How much calcium stearate will be obtained if 28.4 g of stearic acid
melt with enough quicklime?
2. Rate of raw material consumption to produce 1 ton of ethyl acetate
is 0.85 t of acetic acid and 0.652 t of ethyl alcohol (in terms of
100%). Calculate the ester yield as a percentage of theoretical.
3. Anhydrous formic acid weighing 69 kg with a yield of 69% is obtained from
sodium formate by the action of H2SO4, and formate - by the reaction of NaOH with carbon monoxide
gas (when heated, under pressure). Determine the required volume (no.
y.) gas.
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4. Calculate the mass of sodium hydroxide required for neutralization
200 g of 9% acetic acid solution.
Option 10
1. What substance and what mass is formed when chlorine acts on
acetic acid weighing 1.2 tons?
2. When 0.76 g of benzyl alcohol reacts with 0.28 g of formic
acid produces a jasmine-scented product. Find the mass of the product
if the loss in synthesis is 20%.
3. When oxidizing a saturated monohydric alcohol, ROH is obtained
carboxylic acid with a yield of 80%. When exposed to excess Zn
4.48 liters of hydrogen were released. What acid and what mass was obtained?
How much and what kind of alcohol was required for the reaction, if during dehydration
Isobutylene is formed from the starting alcohol?
4. When heating 25.8 g of a mixture of ethyl alcohol and acetic acid in
in the presence of H2SO4, 14.08 g of ester was obtained, and when burning this
The same mass of the initial mixture produced 23.4 g of water. Find the mass fraction
starting mixture and calculate the ester yield.
Option 11
1. When hydrogenating acrylic acid weighing 14.4 g, we used
hydrogen obtained from partial cracking of methane with a volume of 4 liters (no.).
What mass of propionic acid was formed and which of the initial
Did you take too much of the substances?
2. How much ethyl acetate can be obtained from 30 g of acetic acid
acid, taking the yield of ester equal to 85% of theoretical?
3. A mixture of butyl alcohol and propionic acid was treated with excess
aqueous NaHCO3 solution. The volume of CO2 released in this case is 15 times higher
less than the volume of CO2 formed during complete combustion of the same
amount of the original mixture. Find the mass fraction of the original mixture
compounds, if 48.16 liters of O2 are required for its combustion.
412
4. Calculate the volume of hydrogen (n.u.) that will be released during the action
magnesium weighing 60 g per acetic acid.
Option 12
1. What is the mass of the reaction product (at 80% yield) obtained at
interaction of a 40% acetic acid solution with a volume of 240 ml (ρ = 1.05
g/cm3
) and 90% methanol with a volume of 120 ml (ρ = 0.7 g/cm3
)?
2. One mole of the primary monohydric alcohol ROH was oxidized to
the corresponding carboxylic acid. The same amount of ROH was subjected
dehydration, then hydration, resulting in an isomeric
original alcohol. From this alcohol and acid an ester was formed, with
complete combustion of which produced 67.2 liters of CO2. What structure does it have?
ester, if its yield in the esterification reaction is 50%,
Are the other reactions quantitative?
3. A mixture of benzoic acid and phenol was treated with bromine water until
stopping discoloration, which took 1.5 kg of bromine water with ω(Br2) =
3.2%, then a 10% aqueous solution of NaOH (ρ = 1.11 g/ml) with a volume of 180.2 ml.
Find the mass fractions of acid and phenol in the original mixture.
4. How many moles of soda ash will be required to react with
stearic acid weighing 28.4 g and what amount of sodium stearate
will it work?
Option 13
1. During the esterification reaction, an 80% solution of methyl alcohol reacted
weighing 30 g and methacrylic acid CH2=C(CH3)-COOH amount
substances 0.6 mol. What is the mass of the resulting ester (methyl methacrylate)?
2. For complete hydrolysis of a mixture of ethyl esters of acetic and propionic acid
acids required 40 g of 20% NaOH solution. When burning the same
amount of starting substances, 20.16 liters of CO2 were formed. Define
mass fractions of esters in the mixture.
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3. There are three test tubes with oleic acid, stearic acid,
glycerin. What chemical reactions can be used to determine each of the
of the listed substances? What mass of glycerin will be required to obtain
89 g glyceryl tristearate?
4. Derive the molecular formula of an organic substance, if known
that ω(C) = 48.65%; ω(O) = 43.24%; ω(Н) = 8.11%, and the relative density
vapor of this substance in air is 2.55.
Option 14
1. What amount of acetic acid was taken for preparation
ethyl acetyl ether, if 70.4 g of the latter were obtained, which
was 80% of the theoretical yield?
2. Calculate the mass of glyceryl triacetate, the product of the reaction between
acetic acid and excess glycerin, if under the influence of carbonate
sodium for the same amount of acetic acid is released 20.16 l (no.)
gas
3. When 30.5 g of benzoic acid reacted with alcohol ROH, we obtained
27.2 g ester. What alcohol was taken if the reaction proceeds with
80% yield?
4. The mixture of propyl alcohol and acetic acid was treated with excess
metal zinc. The gas released in this case is completely
reacted with 15 ml of isoprene (ρ = 0.68 g/ml), turning it entirely into
methylbutene Find the mass fraction of the components of the original mixture if
It is known that in the presence of concentrated sulfuric acid
16.32 g of the corresponding ester were formed (assume that
the esterification reaction was completed by 80%).
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Part VI Carbohydrates
Option 1
1. On a sunny day, due to photosynthesis, a green plant absorbs
air 5 g carbon dioxide per 1 m2
area of its foliage. Calculate
mass (in grams) of glucose that sunflower leaf accumulates per day
whose surface is 1.4 m
2
.
2. How many grams of glucose were subjected to alcoholic fermentation,
proceeded with a yield of 80%, if to neutralize the resulting
this CO2(IV) required 65.57 ml of 20% sodium hydroxide solution
(ran density 1.22)? How many grams of sodium bicarbonate?
formed?
3. From 100 g of glucose we obtained 160 g of glucose pentaacetate. Calculate output
in percentages.
4. What compound and in what quantity is formed during the action
acetic anhydride (taken in excess) per 1 kg of glucose?
Option 2
1. Some organic compound weighing 27 g containing oxygen,
reacts completely with 34.8 g of silver(I) oxide in ammonia solution. At
combustion of the same compound with the volume (in liters, N.U.) consumed
oxygen and the resulting carbon dioxide are the same. Set the title
connections.
2. What mass of glucose is formed from starch weighing 22 tons, if mass
Is the percentage of glucose yield 90% of theoretical?
3. Upon hydrolysis of starch weighing 324 g with a yield of 80%, glucose was obtained,
which was subjected to alcoholic fermentation. Yield of fermentation product
amounted to 75%. As a result of the process, aqueous water was formed
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alcohol solution weighing 600 g. Determine the mass fraction of ethanol in
the resulting solution.
4. As a result of fermentation of glucose, 115 g of alcohol is obtained. What volume
Under normal conditions, the resulting dioxide will take up
carbon?
Option 3
1. Sucrose is hydrolyzed in an acidic environment, and the resulting
glucose - lactic acid fermentation. 54 g of acid are obtained with the yield
80%. What mass (in grams) of sucrose was consumed?
2. As a result of alcoholic fermentation of glucose, ethanol was obtained,
which has been oxidized to acid. When exposed to excess
potassium bicarbonate, gas was released into all the resulting acid
volume 8.96 l (n.u.). Determine the mass of glucose subjected to
fermentation.
3. Glucose was obtained from starch weighing 8.1 g, the yield of which was 70%.
Excess ammonia solution of silver oxide was added to glucose. Which
mass of silver formed in this case?
4. From 100 g of fine sawdust (60% fiber) as a result
hydrolysis when heated with concentrated sulfuric acid solution
received 36 g of glucose. Calculate the percentage yield of the product.
Option 4
1. During alcoholic fermentation of glucose, 460 g of organic
product. What is the mass (in grams) of glucose that reacted?
Also calculate the volume (no.) of the gas released.
2. The mass fraction of starch in potatoes is 20%. What mass
glucose can be obtained from potatoes weighing 1620 kg, if the yield
product is 75%?
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3. To quantify aldoses in the presence of ketoses, use
reaction with iodine and alkali. Write the reaction equation and calculate
weight amount of glucose in solution, if the reaction
0.254 g of iodine entered.
4. From 100 g of pure cotton wool (95% fiber) we obtained 60 g of octaacetate
cellobioses. Calculate the percentage yield.
Option 5
1. From 500 kg of potatoes containing 22% (by weight) starch
glucose and ethanol. Find a lot of products if there is no practical solution
exceeds 76%.
2. After complete combustion of 9 g of carbohydrate in oxygen, 13.2 g of gas and 5.4
g water. Derive the formula of carbohydrate with relative molecular weight
180.
3. What mass of cellulose triacetate can be obtained from wood
waste weighing 1.62 tons, if the ether is obtained with a yield of 75%? Mass fraction
cellulose in wood is 50%.
4. What is the mass fraction (%) of the dissolved substance in the solution,
obtained by dissolving 20 g of sugar in 140 g of water?
Option 6
1. When fermenting glucose weighing 72 g, ethyl alcohol weighing 35 g was obtained.
Determine the mass fraction of ethyl alcohol yield relative to
theoretical.
2. What mass of cellulose and what volume of solution with mass fraction of nitrogen
acid 80% and density 1.46 g/ml must be taken to obtain
trinitrocellulose weighing 990 kg? The yield of trinitrocellulose is
66,7%.
3. During the alcoholic fermentation of glucose, a gas is obtained that reacts with
sodium hydroxide solution with a volume of 60.2 ml and a density of 1.33 g/ml,
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forming a medium salt. Mass fraction of sodium hydroxide in this solution
equal to 30%. What mass of solution with a mass fraction of ethanol of 60% is obtained?
wherein?
4. With complete combustion of 0.75 g of organic matter, 0.56 l was formed
carbon monoxide (IV) (n.o.) and 0.45 ml of water. Relative molecular
the mass of this substance is 180. Determine its chemical formula.
Option 7
1. During the alcoholic fermentation of glucose, a gas was released, the volume of which is equal to
obtained by combustion in air 32 g of methanol. What quantity
monosaccharide (mol) consumed?
2. What mass of corn grains must be taken to obtain alcohol weighing
115 kg, with a mass fraction of ethanol of 96%, if the alcohol yield is 80%?
The mass fraction of starch in corn grains is 70%.
3. From 80 g of finely chopped cotton wool (95% fiber) by hydrolysis at
heating with a concentrated solution of sulfuric acid obtained 38 g
glucose. Calculate the percentage yield of the product.
4. What volume of oxygen was released during photosynthesis (n.a.), if
did the plant absorb 44.8 liters of carbon monoxide (IV)?
Option 8
1. Hydrated cellulose, used for the production of viscose fiber,
obtained in the following way: α-cellulose extracted from wood
treated with caustic soda, resulting in the formation of an alkaline
cellulose, which with carbon disulfide produces cellulose xanthate,
transforming after a series of operations into hydrated cellulose. Calculate
daily need for wood for a plant with a capacity of 120 tons
fiber per day, considering that from 1 m
3
about 200 kg of wood is obtained
cellulose.
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2. From 100 g of deashed filter paper (fiber) as a result
hydrolysis when heated with concentrated hydrochloric acid (41 - 42%,
HC1) received 56 g of glucose. Calculate the percentage yield of the product.
3. Calculate the mass of silver resulting from the interaction of glucose
weighing 54 g with an ammonia solution of silver oxide. Mass fraction of yield
is 75%.
4. What mass of glucose was taken if ethylene was obtained in volume
11.2 l (no.), and the mass fraction of ethylene yield was 50%?
Option 9
1. What mass of lactic acid is formed during lactic acid fermentation
glucose weighing 40 g, if the mass fraction of impurities in glucose is
10%?
2. The mass fraction of cellulose in wood is 50%. What mass
alcohol can be obtained from the fermentation of glucose, which
is formed during the hydrolysis of sawdust weighing 810 kg? Take account,
that alcohol is released from the reaction system in the form of a solution with
mass fraction of water 8%. Ethanol yield due to production
losses amount to 70%.
3. The plant absorbed carbon monoxide (IV) in the process of photosynthesis
33.6 l (N.S.). What amount of glucose was formed in this case?
4. Calculate the mass of methane taken, if the resulting hydrogen
reduced glucose weighing 36 g.
Option 10
1. During the fermentation of glucose, we obtained ethanol weighing 354 g, the yield of which was
amounted to 78%. What mass of glucose was fermented?
2. What volume of air, the volume fraction of oxygen in which is 21%,
required for complete oxidation of glucose weighing 45 g? Calculate volume
under normal conditions.
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3. How much glucose can be obtained from 1 ton of potatoes, which contains
22% starch if the glucose yield is 80% of theoretical?
4. Calculate the mass of sucrose that has undergone hydrolysis, taking into account the fact that
From the resulting glucose, lactic acid weighing 54 g was obtained at
mass fraction yield 60%.
Option 11
1. With lactic acid fermentation of glucose weighing 72 g, lactic acid was obtained
acid weighing 60 g. What is the mass fraction of lactic acid yield by
relation to the theoretical?
2. What mass of reaction products is formed when glucose is heated
weighing 36 g with copper(II) hydroxide weighing 25 g?
3. What volume of carbon monoxide (IV) will be released during alcoholic fermentation
glucose weighing 270 kg? Calculate the volume under normal conditions.
4. By hydrolysis of sawdust weighing 324 g, glucose was obtained.
Calculate the mass of alcohol formed during its fermentation if
the mass fraction of yield is 60%.
Option 12
1. Calculate how much metallic silver can be obtained with
interaction of 18 g of glucose with an ammonia solution of silver oxide, if
the product yield is 75%. What volume of gas (n.a.) will be released when
alcoholic fermentation of the same amount of glucose, if we assume that
Is the process only 75% complete?
2. What mass of starch must be hydrolyzed so that the resulting
glucose during lactic acid fermentation, lactic acid is formed
weighing 108 g? The yield of starch hydrolysis products is 80%, the product
glucose fermentation - 60%.
3. Calculate the mass of glucose obtained from the hydrolysis of sucrose with a mass
68.4 g, if the mass fraction of the product yield was 70%.
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4. What is the mass of acetic acid spent (maximum) on
reaction with a glucose solution weighing 50 g with a mass fraction of dissolved
substances 10%?
Option 13
1. What mass of fiber was hydrolyzed if glucose was formed?
weighing 32 kg, and the mass fraction of the product yield is 82%?
2. Fermentation of glucose produced 276 g of ethanol. What is the mass of carbohydrate
if the product yield is 80%?
3. What is the volume of gas (no.) released during alcoholic fermentation of glucose,
if the mass of the resulting alcohol is 69 g?
4. When fermenting glucose weighing 180 g, lactic acid weighing
153 g. Calculate the mass fraction of the product yield.
Option 14
1. What is the mass fraction of the yield of dinitrocellulose in relation to
theoretical, if dinitro fiber is obtained from fiber weighing 2.8 kg
weighing 3.3 tons?
2. During daylight hours, a beet leaf with an area of 1 dm2 can absorb the oxide
carbon (IV) with a volume of 44.8 ml (n.o.). What mass of glucose is formed when
is this as a result of photosynthesis?
3. When adding glucose solution to the blue precipitate of copper (II) hydroxide
the color changed to red. Write down the reaction equation and
Calculate the mass of the resulting precipitate if glucose is taken with a mass of 18 g.
4. What is the mass of calcium carbonate formed by passing the oxide
carbon (IV) through lime water, if carbon monoxide (IV) is obtained from
fermentation of glucose weighing 36 g?
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Part VII Nitrogen-containing
Option 1
1. When dehydrogenating a mixture of cyclohexane and cyclohexene into benzene
hydrogen is released in an amount sufficient for complete reduction
36.9 g nitrobenzene in aniline. Find the mass fraction of the components
initial mixture, if it is known that such an amount of this mixture can
decolorize 480 g of 10% bromine solution.
2. Upon combustion of 9 g of primary amine, 2.24 liters of nitrogen (n.e.) were released.
Determine the molecular formula of the amine.
3. 6.72 liters of methane during chlorination completely turned into equimolar
a mixture of three compounds whose hydrogen vapor densities are
respectively equal to 77, 59.75 and 42.5. What compounds are in the mixture?
Determine what mass of a 20% aqueous solution of methylamine can
react with the resulting HCl.
4. Determine the mass of propyl ester of α-aminopropionic acid,
formed by the interaction of propyl alcohol weighing 18 g with α-
aminopropionic acid.
Option 2
1. What organic compound has the composition: C - 53.3%, H - 15.6%, N
31.1% and hydrogen vapor density 22.5?
2. 16.6 g of a mixture of ethanol and propanol was treated with excess Na, while
3.36 liters of hydrogen were released. Determine the mass fraction of components
initial mixture of alcohols. What mass of this mixture must be taken to
Using the hydrogen obtained from it, reduce 24.6 g of nitrobenzene to aniline?
3. How much benzene will be required to obtain 17.4 g of aniline hydrobromide
in three stages of synthesis, if the yield at the last stage is quantitative, and at
two previous ones at 50%?
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4. What reaction product and what mass is formed during the interaction
aminoacetic acid weighing 30g with ethyl alcohol?
Option 3
1. Establish the molecular formula of the secondary amine, mass fractions
carbon, hydrogen and nitrogen atoms in which are respectively equal to: 61.0%,
15.3% and 23.7%.
2. Determine in what molar ratios they are present in the mixture
nitrobenzene and toluene, if during the oxidation of the KMnO4 mixture the mass of the initial
the mixture increases by 6 g, and when restored, decreases by 3 g.
3. What mass of benzene will be required to produce by three-stage synthesis
33 g of 2,4,6 - tribromoaniline, if it is known that the yield is at the last stage
quantitative, and in the previous ones 50%?
4. When producing aniline by reducing nitrobenzene, the reaction took place
not complete enough. The aniline distilled off with steam turned out to be contaminated
nitrobenzene. 1/25 of the resulting aniline was burned, gaseous
the reaction products were absorbed by an excess of aqueous KOH solution. At the same time not
0.448 liters of gas were absorbed. The same part of the resulting aniline was processed
25 ml of 20% H2SO4 solution (ρ = 1.14 g/ml), with the formation of 6.88 g
draft. How much aniline was obtained and what is the mass fraction of nitrobenzene
ended up in it?
Option 4
(n.a.) nitrogen.
2. A mixture of benzene and cyclohexane was subjected to dehydrogenation, while
enough hydrogen was released to completely reduce 24.6 g
nitrobenzene. Benzene formed during the reaction and the original benzene
were treated with chlorine under light. Find the mass fraction
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components of the initial mixture, if the mass of the benzene chlorination product
increased by 85.2 g.
3. What volume of air, the volume fraction of oxygen in which is 21%,
required to burn 8 liters (N.O.) of methylamine.
4. Current was passed into a mixture of aminoacetic acid and anhydrous ethanol.
dry HCl, and 1.4 g of solid was formed. What is this
substance? What mass of ethanol reacted?
Option 5
1. Upon combustion, 0.31 g of gaseous organic matter was released
0.224 l of carbon dioxide, 0.45 g of water and 0.112 l of nitrogen. Density of matter
1.384 g/l. Determine the molecular formula of the compound and name it.
2. The gas formed during the production of bromobenzene from benzene was passed into
excess aqueous methylamine solution. When evaporated to dryness
the resulting solution left 11.2 g of solid. Which
amount of benzene was taken if the yield of bromobenzene was 80%?
How many grams of bromobenzene did you get?
3. A mixture weighing 30 g containing aminoacetic acid, acetic
acid and acetaldehyde, for salt formation requires HCl volume
5.38 l (n.s.) or CaO weighing 10.08 g. Calculate the mass fractions of substances in
original mixture.
4. Determine the mass of salt formed during the interaction of β-
aminobutyric acid weighing 20.6 g with sodium hydroxide weighing 9 g.
Option 6
1. When benzene and aniline were burned, 6.94 liters of gaseous
products that, when passed into an excess of aqueous KOH solution, do not
224 ml of gas were absorbed. Find the mass fraction of the components of the original
mixtures.
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2. A mixture of four isomeric organic compounds, each of which
easily reacts with HCl and contains 23.7% nitrogen in the molecule when burned
forms 4.48 liters of nitrogen. Determine the structure of these compounds and mass
original mixture.
3. What volume of ammonia is required to react with chloroacetic acid
weighing 18.9 g (reaction with the group - COOH is excluded)?
4. How many grams of calcium carbide containing 10% impurities,
necessary to obtain 2 mol by the corresponding reactions
aminoacetic acid?
Option 7
1. What mass of aminoacetic acid and butyl alcohol is consumed for
obtaining butyl ester of aminoacetic acid weighing 23.4 g?
2. The gas released during the production of bromobenzene from 7.8 g of benzene is
reacted completely with an equivalent amount of methylamine,
located in 50 g of aqueous solution. Determine the mass fraction
methylamine in solution if 80% benzene has entered the bromination reaction.
3. To react 38.7 g of a mixture of benzoic acid and sulfate
primary amine (R-NH2 . H2SO4) required 144 ml of 10% aqueous
NaOH solution (ρ = 1.1 g/ml). Determine which amine sulfate was in
mixture, if it is known that when processing the same mass of the original mixture
an excess of an aqueous solution of BaCl2 produces 23.3 g of precipitate.
4. At a nitrogen fertilizer plant from 6 tons of ammonia and 10 tons of carbon dioxide at
pressure 200 atm. and heating, 10 tons of urea were obtained. What percentage
does this amount to a theoretically possible yield? What substance and
how much was taken in excess?
Option 8
1. Gaseous combustion products of a mixture of benzene and aniline were passed into
excess barite water, resulting in the formation of 59.4 g of sediment.
Determine the mass fraction of the components of the initial mixture if, at
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processing the same amount of mixture with dry HCl can release 2.59 g
draft.
2. The mass fraction of oxygen in a monobasic amino acid is 42.67%.
Determine the molecular formula of the acid.
3. Determine the volume of ammonia consumed in obtaining aminoacetic acid
acid weighing 600 g with a mass fraction of yield of 80%.
4. What mass of salt is formed during the interaction of potassium hydroxide with α-
aminopropionic acid weighing 20 g, if the mass fraction of impurities in
acid 11%?
Option 9
1. A mixture of methylamine hydrochloride and ammonium chloride was treated with aqueous
NaOH solution and heated. The released gas was burned, and the resulting
Gaseous products were passed into excess lime water. Wherein
10 g of sediment were obtained. The same amount of the original mixture was dissolved in
water and treated with silver nitrate. In this case, 43 g of sediment was obtained.
Determine the mass fraction of the components of the initial mixture.
2. To neutralize aniline hydrochloride obtained by reduction
nitrobenzene, 18% NaOH solution was used, 2 times more than for
neutralization of the gaseous bromination product of 39 g of benzene. Exit
at the bromination stage 60%. Determine the mass of the hydrochloride taken
aniline.
3. What is the volume of 90% methanol (density 0.8 g/cm3
) is necessary for the reaction with
aminoacetic acid amount of substance 2 mol?
4. The hydrolysis of urea produced 224 ml of ammonia (n.a.). How many
Was urea hydrolyzed?
Option 10
1. During the combustion of a secondary amine with a symmetrical structure,
0.896 l of carbon dioxide, 0.99 g of water and 0.112 l (no.) nitrogen. Install
molecular formula of this amine.
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2. A mixture of propane and methylamine was passed through an excess of 2 M HCl solution,
at the same time, the volume of the mixture decreased three times. The same volume of the original
the mixtures were burned, and the combustion products were passed into an excess of barite water,
from which 98.5 g of sediment was released. Determine the mass fraction
components of the original mixture.
3. What mass of salt is formed during the interaction of α-aminoacetic
acid weighing 30.3 g with hydrochloric acid weighing 12 g?
4. Determine the volume of 96% ethanol with a density of 0.8 g/ml required for
esterification of 3 g of glycine, if the alcohol is taken with 100% excess.
Option 11
1. When reducing nitrobenzene weighing 73.8 g, we obtained aniline weighing
48 g. Determine the yield of the product.
2. The products of complete combustion of a mixture of propane and methylamine were processed
excess barite water. In this case, 137.9 g of sediment was formed.
The remaining gas that was not absorbed by barite water was passed over
hot copper spiral, after which the volume of gas turned out to be 2.5 times
less than the volume of the original mixture of propane and methylamine. Define
mass fraction of the components of the initial mixture.
3. What mass of salt is formed during the interaction of aminoacetic acid
weighing 30 g with a solution of sulfuric acid weighing 250 g, mass fraction of H2SO4 in
Which one is 10%?
4. What volume of nitrogen is formed when ethylamine weighing 5.4 g is heated?
Calculate the volume at n. u.
Option 12
1. 2.36 g of primary amine were burned. The resulting gases were passed through
excess NaOH solution. Gas not absorbed by alkali has a volume of 448 ml
(Well.). Determine the formula of the amine and all its isomers.
2. Dry gaseous HCl was passed into the mixture of benzene, phenol and aniline.
In this case, 3.89 g of precipitate was released, which was filtered. Benzene
filtrate, washed with a small amount of water to remove residual HCl,
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treated with a 10% aqueous solution of NaOH (ρ = 1.11 g/ml), which was used
reaction 7.2 ml. Find the mass fraction of the components of the original mixture if
when burning the same amount, 20.5 liters should be formed
gaseous products.
3. What mass of aminoacetic acid can be obtained from 46 g of ethanol?
How many liters of NH3 (N.O.) will be required for this purpose? Write a diagram
conversion of ethanol to aminoacetic acid.
4. How much 2-nitropropane should be taken to catalytically
by reduction obtain 1 kilogram of 2-aminopropane, if the yield of amine
is 92% of the theoretical?
Option 13
1. Establish the molecular formula of a tertiary amine if it is known that
upon its combustion, 0.896 liters of carbon dioxide, 0.99 g of water and 0.112 liters of
(n.a.) nitrogen.
2. When processing a mixture of aniline hydrochloride and benzoic acid
an excess of an aqueous solution of NaHCO3 released 1.12 liters of gas. If
Burn the resulting aniline, then 336 ml of nitrogen should be formed. Find
mass fraction of mixture components.
3. What mass of propyl alcohol will be required to obtain 8.9 g of alanine
(α - aminopropionic acid), if it is known that at the first stage the yield
90%, in the second - 80%, the remaining stages are carried out with quantitative
way out? Write a scheme for the synthesis of alanine from propyl alcohol. Which
substance and what mass is formed if a mixture of alanine and anhydrous
ethanol passed a current of dry HCl?
4. When urea is heated to 190ºC, biuret is formed and this is released
the amount of ammonia that, when passed into a half-liter flask with
water, forms 3.4% ammonia. How much urea enters
reaction?
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Option 14
1. When treating 4.02 g of a mixture of nitrobenzene and aniline with dry gaseous
HCl released 3.9 g of sediment. What is the minimum mass of zinc and what
a minimum volume of 10% hydrochloric acid (ρ = 1.05 g/ml) will be required for
complete restoration of this mixture? (all reactions are quantitative).
2. What mass of ethanol will be required to obtain 18.6 g of aniline, if
It is known that at the stage of benzene production the yield is 30%, the remaining stages
pass with a yield of 80%?
3. When 2.4 g of an organic compound is burned, 1.44 g of water is obtained,
896 ml (n.s.) carbon dioxide and 0.04 mol nitrogen. Derive the formula
source connection and give it a name.
4. Determine the molar mass and structure of the aminoacetic ester
acid if it is known to contain 15.73% nitrogen.
- When 1.48 g of saturated monohydric alcohol interacted with sodium metal, hydrogen was released in an amount sufficient to hydrogenate 224 ml of ethylene (n.s.). Determine the molecular formula of alcohol.
Show 1) 2C n H 2 n +1 OH + 2Na → 2C n H 2 n +1 ONa + H 2
2) C 2 H 4 + H 2 → C 2 H 6 n(C 2 H 4) = 0.224/22.4 = 0.01 mol.
According to equation (2) n(C 2 H 4) = n(H 2).
According to equation (1) n(C n H 2 n +1 OH) = 2n(H 2) = 0.02 mol.
M(C n H 2 n +1 OH) = m/n = 1.48/0.02 = 74 g/mol.
M(C n H 2 n +1 OH) = 14n+18
14n+18 = 74
n= 4
C 4 H 9 OH - butanol - When a substance that does not contain oxygen is completely burned, nitrogen and water are formed. The relative vapor density of this substance with respect to hydrogen is 16. The volume of oxygen required for combustion is equal to the volume of nitrogen released. Determine the general formula of the compound and the true formula of the substance.
Show N x H y + 0.25yO 2 → 0.5yH 2 O + 0.5xN 2
M(H x N y)= D H 2 * 2 = 16*2 = 32 g/mol.
Since the volumes of oxygen and nitrogen are equal, then 0.25y=0.5x
y=2x => x: y= 0.25: 0.5 = 1: 2
simplest formula NH 2
M(NH 2) = 16 g/mol
M(H x N y)= D H 2 * 2 = 16*2 = 32 g/mol. – twice the molar mass of the simplest formula =>
True formula N 2 H 4 - Determine the molecular formula of the alkene and the product of its reaction with 1 mol of hydrogen bromide if this monobromo derivative has a relative density in air of 4.24. Indicate the name of one isomer of the parent alkene.
- Determine the molecular formula of a monochloroalkane containing 38.38% chlorine. Give graphic formulas and names of all compounds that correspond to this formula.
Show ω(Сl) = M(Cl)/M(С n H 2 n +1 Cl)
M(C n H 2 n +1 Cl) = 35.5/0.3838 = 92.5 g/mol.
M(C n H 2 n +1 Cl) = 14n+ 36.5 g/mol.
14n+ 36.5 = 92.5
n= 4 => molecular formula C 4 H 9 Cl – chlorobutane - Upon combustion of 9 g of saturated secondary amine, 2.24 liters of nitrogen and 8.96 liters of carbon dioxide were released. Determine the molecular formula of the amine.
Show R 1 –NH–R 2 + O 2 → CO 2 + H 2 O +N 2
n(N 2)=V/Vm= 2.24/22.4 = 0.1 mol => n(N)=0.2 mol
n(CO 2)=V/Vm= 8.96/22.4 = 0.4 mol => n(C) = 0.4 mol
n(C) : n(N) =0.4: 0.2 = 2: 1 => molecular formula of the secondary amine CH 3 NHCH 3 - dimethylamine. - When 11.6 g of saturated aldehyde interacted with an excess of copper (II) hydroxide upon heating, a precipitate weighing 28.8 g was formed. Derive the molecular formula of the aldehyde.
- Upon combustion of 9 g of primary amine, 2.24 liters of nitrogen (n.o.) were released. Determine the molecular formula of the amine and give its name.
- When 1.74 g of alkane reacted with bromine, 4.11 g of a monobromo derivative was formed. Determine the molecular formula of the alkane.
- When 0.672 l of alkene (n.s.) reacts with chlorine, 3.39 g of its dichloro derivative is formed. Determine the molecular formula of the alkene, write down its structural formula and name.
- When the same amount of alkene reacts with different hydrogen halides, 7.85 g of a chlorine derivative or 12.3 g of a bromo derivative are formed, respectively. Determine the molecular formula of the alkene, write down its name and structural formula.
- When the same amount of alkene reacts with halogens, 11.3 g of a dichloro derivative or 20.2 g of a dibromo derivative are formed, respectively. Determine the molecular formula of the alkene, write down its name and structural formula.
- Establish the molecular formula of an alkene that does not have geometric isomers, if it is known that 1.5 g of it can add 0.6 l (n.s.) of hydrogen. Write down the names of alkenes that satisfy the conditions of the problem.
- When a primary monohydric alcohol containing 60% carbon and 13.3% hydrogen interacted with an organic acid, a substance was formed whose vapor density for hydrogen was 58. Determine the molecular formula of each of the substances participating in the reaction and give them names.
- Determine the molecular formula of dibromoalkane containing 85.11% bromine.
- Determine the molecular formula of an alkene, the hydration of which produces alcohol, the vapor of which is 2.07 times heavier than air.
- Determine the molecular formula of a saturated tertiary amine containing 23.73% nitrogen by mass.
- The mass of an unknown volume of air is 0.123 g, and the mass of the same volume of gaseous alkane is 0.246 g (under the same conditions). Determine the molecular formula of the alkane.
- An organic substance weighing 1.875 g occupies a volume of 1 liter (n.s.). When 4.2 g of this substance is burned, 13.2 g of CO2 and 5.4 g of water are formed. Determine the molecular formula of the substance.
- A saturated monobasic carboxylic acid weighing 11 g was dissolved in water. To neutralize the resulting solution, 25 ml of sodium hydroxide solution was required, the molar concentration of which was 5 mol/l. Determine the formula of the acid.
- Establish the molecular formula of an alkene if it is known that the same amount of it, interacting with halogens, forms, respectively, either 56.5 g of a dichloro derivative or 101 g of a dibromo derivative.
- As a result of combustion of 1.74 g of an organic compound, 5.58 g of a mixture of CO2 and H2O was obtained. The amounts of CO2 and H2O substances in this mixture turned out to be equal. Determine the molecular formula of an organic compound if its relative oxygen density is 1.8125.
- Determine the molecular formula of an alkene if it is known that 0.5 g of it can add 200 ml (n.s.) of hydrogen.
- Establish the molecular formula of an alkene if it is known that 1.5 g of it can add 600 ml (n.s.) of hydrogen chloride.
- When 22 g of saturated monobasic acid reacted with an excess of sodium bicarbonate solution, 5.6 l (n.s.) of gas was released. Determine the molecular formula of the acid.
- When 25.5 g of saturated monobasic acid reacted with an excess of sodium bicarbonate solution, 5.6 l (n.s.) of gas was released. Determine the molecular formula of the acid.
Show C n H 2n+1 COOH + NaHCO 3 = C n H 2n+1 COONa + H 2 O + CO 2
n(CO 2) =5.6: 22.4 = 0.25 mol
n(CO 2) = n(C n H 2n+1 COOH) = 0.25 mol
M(C n H 2 n+1 COOH) = 25.5/0.25 = 102 g/mol
M(C n H 2n+1 COOH) = 12n + 2n + 1 + 45 = 102
Molecular formula – C 4 H 9 COOH
- Establish the molecular formula of a tertiary amine if it is known that its combustion produced 0.896 l (n.s.) of carbon dioxide, 0.99 g of water and 0.112 l (n.s.) nitrogen.
- During the combustion of a secondary amine of symmetrical structure, 0.896 l (n.s.) of carbon dioxide, 0.99 g of water and 0.112 l (n.s.) of nitrogen were released. Determine the molecular formula of this amine.
- Determine the molecular formula of acetylene hydrocarbon if the molar mass of the product of its reaction with excess hydrogen bromide is 4 times greater than the molar mass of the original hydrocarbon.
- The mass fraction of oxygen in a monobasic amino acid is 42.67%. Determine the molecular formula of the acid.
- A certain ester weighing 7.4 g was subjected to alkaline hydrolysis. In this case, 9.8 g of potassium salt of saturated monobasic acid and 3.2 g of alcohol were obtained. Determine the molecular formula of this ester.
- Determine the molecular formula of an alkyne whose relative vapor density in air is 1.862.
- With complete combustion of the hydrocarbon, 27 g of water and 33.6 l of CO2 (n.s.) were formed. The relative density of the hydrocarbon with respect to argon is 1.05. Determine its molecular formula.
- When 0.45 g of gaseous organic matter was burned, 0.448 l (n.s.) of carbon dioxide, 0.63 g of water and 0.112 l (n.s.) of nitrogen were released. The density of the initial gaseous substance by nitrogen is 1.607. Determine the molecular formula of this substance.
- With complete combustion of 0.59 g of some limiting primary amine, 0.112 liters of nitrogen (n.s.) were released. Determine the molecular formula of this amine.
- The combustion of 1.8 g of some primary amine released 0.448 l (n.s.) of nitrogen. Determine the molecular formula of this amine.
- The combustion of oxygen-free organic matter produced 4.48 liters (n.s.) of carbon dioxide, 3.6 g of water and 3.65 g of hydrogen chloride. Determine the molecular formula of the burnt compound.
- A certain saturated carboxylic monobasic acid weighing 6 g requires the same mass of alcohol for complete esterification. This yields 10.2 g of ester. Determine the molecular formula of the acid.
- An ester weighing 30 g was subjected to alkaline hydrolysis. In this case, 34 g of sodium salt of saturated monobasic acid and 16 g of alcohol were obtained. Determine the molecular formula of this ester.
- When the amine burned, 0.448 l (n.s.) of carbon dioxide, 0.495 g of water and 0.056 l of nitrogen were released. Determine the molecular formula of this amine.
- Establish the molecular formula of a saturated monobasic carboxylic acid, the calcium salt of which contains 30.77% calcium.
- When 22 g of saturated monohydric alcohol interacted with an excess of metallic sodium, 2.8 liters (n.s.) of gas were released. Determine the molecular formula of alcohol.
- When 23 g of saturated monohydric alcohol reacted with an excess of metallic sodium, 5.6 l (n.s.) of gas was released. Determine the molecular formula of alcohol.
- When 30 g of saturated monohydric alcohol reacted with metallic sodium, 5.6 liters (n.s.) of gas were released. Determine the molecular formula of alcohol.
- Establish the molecular formula of an alkene if it is known that as a result of the addition of chlorine to 1.008 l (n.s.) of an alkene, 5.09 g of a dichloro derivative is formed.
- As a result of the reaction of saturated dihydric alcohol weighing 30.4 g with an excess of metallic sodium, 8.96 l (n.s.) of gas was obtained. Determine the molecular formula of the original alcohol.
- When 8.96 l (n.s.) of hydrogen bromide reacted with an equal volume of gaseous amine, a product weighing 50.4 g was obtained. Determine the molecular formula of the amine.
- As a result of fusing the sodium salt of a carboxylic acid with sodium hydroxide, 24.38 g of sodium carbonate and a gaseous organic substance weighing 6.9 g were obtained. Determine the molecular formula of the resulting gaseous compound.
- As a result of fusing the sodium salt of a carboxylic acid with sodium hydroxide weighing 4.8 g, sodium carbonate and a gaseous organic substance weighing 3.6 g were obtained. Determine the molecular formula of the resulting gaseous compound.
- As a result of fusing the sodium salt of a carboxylic acid with sodium hydroxide, 46.64 g of sodium carbonate and a gaseous organic substance weighing 19.36 g were obtained. Determine the molecular formula of the resulting gaseous compound.
- As a result of fusing the sodium salt of a carboxylic acid with sodium hydroxide weighing 14 g, sodium carbonate and a gaseous organic substance weighing 15.4 g were obtained. Determine the molecular formula of the resulting gaseous compound.
- Alkaline hydrolysis of 37 g of a certain ester yields 49 g of potassium salt of a saturated monobasic acid and 16 g of alcohol. Determine the molecular formula of the ester.
- Saturated monohydric alcohol was treated with hydrogen chloride. As a result of the reaction, a halogen derivative weighing 39.94 g and 6.75 g of water were obtained. Determine the molecular formula of the original alcohol.
Option 1
1. General formula of alkynes:
1) C n H 2 n 2) C n H 2 n-2 3) C n H 2 n+2 4) C n H 2 n-6
2. Name of the substance, whose formula CH 3 ─ CH 2 ─ CH (CH 3)─ C ≡ CH
1) hexine -1 3) 3-methylhexine 2) 3-methylpentine-1 4) 3-methylpentine-4
3. Type of hybridization
CH 2 ═ C * ═ CH 2
4. What substance molecules do not have π bonds?
1) ethine 2) ethene 3) isobutane 4) cyclopentane
5. Homologues are:
1) methanol and phenol 3) glycerin and ethylene glycol
2) butine-2 and butene-2 4) 2-methylpropene and 2-methylpentane
6. Isomers are:
1) benzene and toluene 3) acetic acid and ethyl formate
2) ethanol and dimethyl ether 4) ethanol and phenol
7. Coloring the mixture glycerol with copper hydroxide (ΙΙ):
1) blue 2) red 3) bright blue 4) purple
8. Aniline from nitrobenzene can be obtained using the reaction:
9. What substances
C 2 H 5 Cl → C 2 H 5 OH → C 2 H 5 ONa
1) KOH, NaCl 2) KOH, Na 3) HOH, NaOH 4) O 2, Na
10. Volume of carbon dioxide, formed by burning 2 liters of butane
1) 2 l 2) 5 l 3) 8 l 4) 4 l
11. Match
A) C 5 H 10 O 5 1) alkynes 2) arenes 3) carbohydrates
B) C 5 H 8 4) ethers
B) C 8 H 10 5) polyhydric alcohols
D) C 4 H 10 O
Phenol reacts with
1) oxygen 2) benzene 3) sodium hydroxide
4) hydrogen chloride 5) sodium 6) silicon oxide (ΙV)
Both ethylene and benzene are characterized by
1) hydrogenation reaction 2) the presence of only π-bonds in molecules
3) sp 2 - hybridization of carbon atoms in molecules 4) high solubility in water
5) interaction with an ammonia solution of silver oxide (I) 6) combustion in air
14. Molecular formula hydrocarbon, the mass fraction of carbon in which
83.3%, and the relative vapor density for hydrogen is 36 ________
15. Write the reaction equations, with which you can implement
transformations according to the scheme
CaC 2 → C 2 H 2 → C 6 H 6 → C 6 H 5 NO 2 → C 6 H 5 NH 2
C 2 H 4 → C 2 H 5 OH
16. Some organic compound weighing 5.8 g, interacting with copper (II) hydroxide, upon heating, formed 14.4 g of copper (I) oxide precipitate. This organic compound reacts by adding sodium hydrosulfite and ethanol.
Final test in organic chemistry, grade 10
Option 2
1. General formula of alkadienes:
2. Name of the substance, whose formula CH 3 ─CH(CH 3)─CH═CH─CH 3
1) hexene-2 2) 4-mnthylpentene-2 3) 2-methylpentene-3 4) 4-methylpentine-2
3. Type of hybridization electron orbitals of carbon atoms in a benzene molecule
1) sp 3 2) sp 3) sp 2 4) not hybridized
4. Only σ-bonds present in the molecule
1) methylbenzene 2) 2-mthylbutene-2 3) isobutane 4) acetylene
Homologues are
1) ethene and methane 2) cyclobutane and butane 3) propane and butane 4) ethine and ethene
The isomers are
1) methylpropane and methylpropene 2) methane and ethane
3) butene-1 and pentene-1 4) methylpropane and butane
7. Coloring the aldehyde mixture
8. Acetaldehyde can be obtained from acetylene using the reaction:
1) Wurtz 3) Kucherov
2) Zinina 4) Lebedeva
9. What substances can be used for sequential
implementation of the following transformations
C 2 H 5 OH → C 2 H 5 Cl → C 4 H 10
1) NaCl, Na 2) O 2, Na 3) HCl, Na 4) HCl, NaOH
10. Volume of oxygen, required to burn 2 liters of methane
1) 2l 2) 10 l 3) 4 l 4) 6 l
11. Match between the molecular formula of an organic
substance and the class to which it belongs
A) C 6 H 6 O 1) monohydric alcohols
B) C 6 H 12 O 6 2) polyhydric alcohols
B) C 3 H 8 O 3) carbohydrates 4) phenols
D) C 2 H 6 O 2 5) carboxylic acids
12. Methanal may react with
1) nitrogen 2) ammonia solution of silver oxide (Ι) 3) phenol
4) toluene 5) sodium 6) hydrogen
13. And for methane, and typical for propene
1) bromination reactions 2) sp-hybridization of carbon atoms in molecules
3) presence of π bonds in molecules 4) hydrogenation reaction
5) combustion in air 6) low solubility in water
14. Molecular formula organic matter, with mass fraction
carbon 51.89%, hydrogen 9.73% and chlorine 38.38%, relative density
its vapor in the air 3, 19 ______
15.. Write the reaction equations, with which you can implement
transformations according to the scheme
C 2 H 6 → C 2 H 5 Cl → C 2 H 5 OH → CH 3 COH → CH 3 COOH
C 2 H 4 → C 2 H 5 Br
16.. A certain organic compound contains 69.6% oxygen by mass. The molar mass of this compound is 1.58621 times the molar mass of air. It is also known that this substance is capable of entering into an esterification reaction with propanol -2. Find the formula of the substance.
Final test in organic chemistry, grade 10
Option 3
1. General formula of alkenes:
1) C n H 2 n 2) C n H 2 n- 3) C n H 2 n+2 4) C n H 2 n-6
2. Name of the substance, whose formula
CH 3 ─CH 2 ─CH(CH 3)─CH(CH 3)─SON
1) 2,3-dimethylbutanal 3) pentanal
2) 2,3-dimethylpentanal 4) 3,4-dimethylpentanal
3. Type of hybridization electron orbitals of the carbon atom, designated
an asterisk in a substance whose formula CH 3 ─C * BUT
1) sp 3 2) sp 3) sp 2 4) not hybridized
4. Number of π bonds in a propyne molecule is equal to
1) 1 2) 3 3) 2 4) 4
5. Homologue of acetic acid acid is acid
1) chloroacetic 2) oleic 3) formic 4) benzoic
6. Isomers are:
1) pentane and pentadiene 2) ethane and acetylene
3) acetic acid and methyl formate 4) ethanol and ethanal
7. Coloring the glucose mixture with copper hydroxide (ΙΙ) (when heated):
1) blue 2) red 3) blue 4) purple
8. Butadiene-1,3 from ethanol can be obtained using the reaction
1) Wurtz 2) Kucherov 3) Zinin 4) Lebedev
9. What substances can be use for sequential
implementation of the following transformations
CH 3 COH → CH 3 COOH → CH 3 COOK
1) O 2, K 2) HCl, KOH 3) Cu and t, KOH 4) HCl, KOH
10. Volume of ethane required to produce 4 liters of carbon dioxide
1) 2l 2) 10 l 3) 4 l 4) 6 l
11. Match between the molecular formula of an organic
substance and the class to which it belongs
A) C 12 H 22 O 11 1) aldehydes
B) C 3 H 8 O 3 2) carboxylic acids
B) C 4 H 8 O 3) polyhydric alcohols
D) C 18 H 36 O 2 4) carbohydrates 5) monohydric alcohols
12. With aminoacetic acid acid can react
1) sodium sulfate 2) hydrogen chloride 3) methane 4) ethanol
5) aniline 6) potassium hydroxide
13. And for ethylene, and for acetylene are characteristic
1) interaction with copper oxide (ΙΙ) 2) the presence of σ- and π-bonds in molecules
3) sp 2 - hybridization of carbon atoms in molecules 4) hydrogenation reaction
5) combustion in air 6) substitution reactions
