Quiz about Chemistry in Class 12

Question 1

Propyne reacts with HOCl which of the following cannot be formed

Accepted Answer

NA

Question 2

Propyne on polymerisation gives

Accepted Answer

NA

Question 3

Propyne to acetone

Accepted Answer

NA

Question 4

Propyne on oxidation with SeO_2 gives

Accepted Answer

NA

Question 5

Propyne is formed by the reaction of

Accepted Answer

NA

Question 6

Propyne and propene can be distinguished by?

Accepted Answer

NA

Question 7

Propyne and propene can be distinguished by

Accepted Answer

NA

Question 8

Propylene is passed through conc. H_2SO_4 and the product thus obtained on hydrolysis with boiling water gives

Accepted Answer

NA

Question 9

Propyl propionate is prepared from which of the following

Accepted Answer

NA

Question 10

Propyl iodide and isopropyl iodide are

Accepted Answer

NA

Question 11

Propyl benzene reacts with bromine in the presence of light and heat to give

Accepted Answer

NA

Question 12

Propose the mechanism of the reaction taking place when  (a). (-)-2-Bromooctane reacts with sodium hydroxide to form (+)-Octane-2-ol.  (b). 2-Bromopentane is heated with KOH (alc). To form alkene.

Accepted Answer

NA

Question 13

Propose mechanism of the reaction taking place when  (a) (-) - 2- Bromooctane reacts with sodium hydroxide to form (+) -octane -2-ol.  (b) 2-Bromopentane is heated with (alc.) KOH to form alkenes.

Accepted Answer

NA

Question 14

Proportions because

Accepted Answer

NA

Question 15

Propiophenone is reduced by NaBH_(4) gives

Accepted Answer

NA

Question 16

Propionic acid with Br_(2)P yields a dibromo product. Its structure would be

Accepted Answer

NA

Question 17

Propionic acid with Br_(2)P yield a dibromo product . Its structure will be

Accepted Answer

NA

Question 18

Propionic acid with BrP yields a dibromo product. Its structure would be

Accepted Answer

NA

Question 19

Propionic acid is obtained from dry ice and what?

Accepted Answer

NA

Question 20

Propionic acid when treated with Br_(2) in the presence of P in sunlight gives

Accepted Answer

NA

Question 21

Propionic acid on bromination in thepresence of red phosphorus gives 2- bromo propionic acids it shows

Accepted Answer

NA

Question 22

Propionic acid is subjected to reduction with hydroiodic acid in the presence of a little P the product formed is

Accepted Answer

NA

Question 23

Propionic acid is obtainedby acidhydrolysis of

Accepted Answer

NA

Question 24

Propionic acid can also be named as

Accepted Answer

NA

Question 25

Propionic acid and KOH reacts to produce which one ofthe folliwng?

Accepted Answer

NA

Question 26

Propionamide when heated with amixture of bromine and caustic alkali wouldgive

Accepted Answer

NA

Question 27

Propionaldoxime is reacted with trifluoroperoxy acetic acid gives

Accepted Answer

NA

Question 28

Propertyof alkaline earthmetals that increases with their atomic number is

Accepted Answer

NA

Question 29

Property of the alkali metals that increases with their atomic number is

Accepted Answer

NA

Question 30

Property of the alkaline earth metals that increases with their atomic number is

Accepted Answer

NA

Question 31

Properties whose values depend only on the concentration of solute particles in solution and not on the identity of the solute are called colligative properties.there may be change in number of moles of solute due to ionisation or association hence these properties are also affected.Number of moles of the product is related to degree of ionisation or association by van Hoff factor i given by i=[1+(n-1)alpha] for dissociation where n is the number of products (ions or molecules ) obtained per mole of the reactant.  & i=[1+(1n-1)alpha] for association  where n is number of reactant particles associated to give 1 mole product.A dilute solution contains t moles of solute X in 1 kg of solvent with molal elevation constant K_b.The solute dimerises in the solution according to the following equation.The degree of association is alpha.  2X hArr X_2  The equilibrium constant for the process can be expressed as

Accepted Answer

NA

Question 32

Properties whose values depend only on the concentration of solute particles in solution and not on the identity of the solute are called colligative properties.there may be change in number of moles of solute due to ionisation or association hence these properties are also affected.Number of moles of the product is related to degree of ionisation or association by van Hoff factor i given by i=[1+(n-1)alpha] for dissociation where n is the number of products (ions or molecules ) obtained per mole of the reactant.  & i=[1+(1n-1)alpha] for association  where n is number of reactant particles associated to give 1 mole product.A dilute solution contains t moles of solute X in 1 kg of solvent with molal elevation constant K_b.The solute dimerises in the solution according to the following equation.The degree of association is alpha.  2X hArr X_2  The colligaive properties observed will be

Accepted Answer

NA

Question 33

Properties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to homegenous solution. These are called colligative properties. Applications of colligative properties are very useful in day to day life. One of its exaples is the use of ethylene glycol and water mixtue as anti-freezing liquid in the radiators of automobiles. A solution M is prepared by mixing ehanol and water. The mole fraction of ethanol in the mixture is 0.9 Given.  K_(f)of water=1.86 K kg mol^(-1)  K_(f)of ethanol = 2.0 K kg mol^(-1) K_(b)for water =0.52 K kg mol^(-1)  K_(b) of ethanol=1.2 K kg mol^(-1)  T_(f)(water)=273 K  T_(f)(ethanol)=155.7 K  T_(b)^(@) (water)=373 K  T_(b)^(@)(ethanol)=351.5 K  P^(@)(water)32.8 mm Hg.  P^(@)(ethanol)=40 mmHg  M(ethanol)==46 g mol^(-1)  M(water)=18g mol^(-1)  In answering the following quesion consider the solutions to be ideal dilute solutions ans solute to be non-voltile and non-dissoviative.  (7) water is added to the solution M such that the mole fraction so wter in solution becomes 0.9. The boiling point of solution is

Accepted Answer

NA

Question 34

Properties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to homegenous solution. These are called colligative properties. Applications of colligative properties are very useful in day to day life. One of its exaples is the use of ethylene glycol and water mixtue as anti-freezing liquid in the radiators of automobiles. A solution M is prepared by mixing ehanol and water. The mole fraction of ethanol in the mixture is 0.9 Given.  K_(f)of water=1.86 K kg mol^(-1)  K_(f)of ethanol = 2.0 K kg mol^(-1) K_(b)for water =0.52 K kg mol^(-1)  K_(b) of ethanol=1.2 K kg mol^(-1)  T_(f)(water)=273 K  T_(f)(ethanol)=155.7 K  T_(b)^(@) (water)=373 K  T_(b)^(@)(ethanol)=351.5 K  P^(@)(water)32.8 mm Hg.  P^(@)(ethanol)=40 mmHg  M(ethanol)==46 g mol^(-1)  M(water)=18g mol^(-1)  In answering the following quesion consider the solutions to be ideal dilute solutions ans solute to be non-voltile and non-dissoviative.  (5) The freezing point of solution M is

Accepted Answer

NA

Question 35

Properties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to homegenous solution. These are called colligative properties. Applications of colligative properties are very useful in day to day life. One of its exaples is the use of ethylene glycol and water mixtue as anti-freezing liquid in the radiators of automobiles. A solution M is prepared by mixing ehanol and water. The mole fraction of ethanol in the mixture is 0.9 Given.  K_(f)of water=1.86 K kg mol^(-1)  K_(f)of ethanol = 2.0 K kg mol^(-1) K_(b)for water =0.52 K kg mol^(-1)  K_(b) of ethanol=1.2 K kg mol^(-1)  T_(f)(water)=273 K  T_(f)(ethanol)=155.7 K  T_(b)^(@) (water)=373 K  T_(b)^(@)(ethanol)=351.5 K  P^(@)(water)32.8 mm Hg.  P^(@)(ethanol)=40 mmHg  M(ethanol)==46 g mol^(-1)  M(water)=18g mol^(-1)  In answering the following quesion consider the solutions to be ideal dilute solutions ans solute to be non-voltile and non-dissoviative.  (6) The vapour pressure of solution M is

Accepted Answer

NA

Question 36

A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9  Given Freezing point depression constant of water  (K_(f)^(water)=1.86 K kg mol^(-1))  Freezing point depression constant to ethanol  (K_(f)^(ethanol))=2.0 K kg mol^(-1))  Boiling point elevation constant of water  (K_(b)^(water))=0.52 K kg mol^(-1)) Boiling point elevation constant of ethanol  (K_(b)^(ethanol))=1.2 K kg mol^(-1))  Standard freezing point of water = 273 K Standard freezing point of ethanol = 155.7 K Standard boilingpoint of water = 373 K Standard boilingpoint of ethanol = 351.5 K Vapour pressure of pure water =32.8 mm Hg Vapour pressure of pure ethanol =40 mm Hg  Molecular weight of water =18 g mol^(-1) Molecular weight of ethanol =46 g mol^(-1) In anwering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative.  Water is added to the solution M such that the mole fraction of water in the solution becomes 0.9. The boiling point of this solution is

Accepted Answer

NA

Question 37

A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9  Given Freezing point depression constant of water  (K_(f)^(water)=1.86 K kg mol^(-1))  Freezing point depression constant to ethanol  (K_(f)^(ethanol))=2.0 K kg mol^(-1))  Boiling point elevation constant of water  (K_(b)^(water))=0.52 K kg mol^(-1)) Boiling point elevation constant of ethanol  (K_(b)^(ethanol))=1.2 K kg mol^(-1))  Standard freezing point of water = 273 K Standard freezing point of ethanol = 155.7 K Standard boilingpoint of water = 373 K Standard boilingpoint of ethanol = 351.5 K Vapour pressure of pure water =32.8 mm Hg Vapour pressure of pure ethanol =40 mm Hg  Molecular weight of water =18 g mol^(-1) Molecular weight of ethanol =46 g mol^(-1) In anwering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative.  The vapour pressure of the solution M is

Accepted Answer

NA

Question 38

A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9  Given Freezing point depression constant of water  (K_(f)^(water)=1.86 K kg mol^(-1))  Freezing point depression constant to ethanol  (K_(f)^(ethanol))=2.0 K kg mol^(-1))  Boiling point elevation constant of water  (K_(b)^(water))=0.52 K kg mol^(-1)) Boiling point elevation constant of ethanol  (K_(b)^(ethanol))=1.2 K kg mol^(-1))  Standard freezing point of water = 273 K Standard freezing point of ethanol = 155.7 K Standard boilingpoint of water = 373 K Standard boilingpoint of ethanol = 351.5 K Vapour pressure of pure water =32.8 mm Hg Vapour pressure of pure ethanol =40 mm Hg  Molecular weight of water =18 g mol^(-1) Molecular weight of ethanol =46 g mol^(-1) In anwering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative.  The freezing point of the solution M is

Accepted Answer

NA

Question 39

Properties such as boiling point freezing point and vapour pressure of a pure solvent change when solution molecules ae added to get homogeneous solution. These are called colligative properties. Application colligative properties are very useful in day-to-day life. One of its example is the use of ethylene glycol and water mixture as anti-freezing liquid in the radiator of automobiles  A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9 Given Freezing point depression of water (K_(f)^(water))=1.86K kg mol^(-1)  Freezing point depression constant of ethanol (K_(f)^(ethanol)=2.0K kg mol^(-1)  Boiling point elevation constant of water (K_(b)^(water)=0.52K kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol)=1.2K kg mol^(-1)  Standard freezing point of water=273K  Standard freezing point of ethanol=155.7K  Standard boiling point of water =373K  Stadndard boiling point of ethanol =351.5K  Vapour pressure of pure water =32.8mm Hg Vapour pressure of pure ethanol=40mm Hg  Molecular weight of water =18 g mol^(-1)  Molecular weight of ethanol =46g mol^(-1)  In aswering the following questions consider the solution to be ideal dilute solutions and solutes to be non volatile and non-dissociative.  the Henrys law constant for the solubility of N_(2) gas in water jat 298K is 1.0xx10^(5) atm. The mole fraction of N_(2) in air 0.8. The number of moles of N_(2) from air dissoved in 10 moles of water of 298K and 5 atm pressure is

Accepted Answer

NA

Question 40

Properties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. one of its examples is the use of ethylene glycol adn water mixtures as anti-freezing liquid in the radiator of automobiles. A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9.  Given Freezing point depression constant of water (K_(f)^(water)) = 1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (K_(f)^(ethanol)) = 2.0 K kg mol^(-1) Boiling point elevation constant of water (K_(b)^(water)) = 0.52 K kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol)) = 1.2 K kg mol^(-1)  Standard freezing point of water = 273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water = 373 K  Standard boiling point of ethanol = 351.5 K  Vapour pressure of pure water = 32.8 mm Hg  Vapour pressure of pure ethanol = 40 mm Hg  Molecular weight of water=18 g mol^(-1)  Molecular weight of ethanol = 46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative. The vapour pressure of the solution M is

Accepted Answer

NA

Question 41

Properties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. one of its examples is the use of ethylene glycol adn water mixtures as anti-freezing liquid in the radiator of automobiles. A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9.  Given Freezing point depression constant of water (K_(f)^(water)) = 1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (K_(f)^(ethanol)) = 2.0 K kg mol^(-1) Boiling point elevation constant of water (K_(b)^(water)) = 0.52 K kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol)) = 1.2 K kg mol^(-1)  Standard freezing point of water = 273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water = 373 K  Standard boiling point of ethanol = 351.5 K  Vapour pressure of pure water = 32.8 mm Hg  Vapour pressure of pure ethanol = 40 mm Hg  Molecular weight of water=18 g mol^(-1)  Molecular weight of ethanol = 46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative. The freezing point of the solution M is

Accepted Answer

NA

Question 42

Properties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Application of colligative properties are very useful in day- to - day life. One of its examples is the use of ethylene glycol and water mixture as anti-freezing liquid in the radiator of automobiles.  A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9.  Given Freezing point depression constant of water (K_(f)^(water))=1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (e_(f)^(ethanol))=2.0 K kg mol^(-1)  Boiling point elevation constant of water (K_(b)^(water))=0.52 K kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol))=1.2 K kg mol^(-1)  Standard freezing point of water = 273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water = 373 K  Standard boiling point of ethanol = 351.5 K  Vapour pressure of pure water = 32.8 mm Hg  Vapour pressusre of pure ethanol = 40 mm Hg  Molecular weight of water = 18 g mol^(-1)  Molecular weight of ethanol = 46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative.  Water is added to the solution M such that the mole fraction of water in the solution becomes 0.9. The boiling of the solution is

Accepted Answer

NA

Question 43

Properties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogenous solution. These are called colligative properties. Application of colligative properties are very useful in day-to-day life. One of its example is the use of ethylene glycol and water mixture as anti-freezing liquid in the radiator of automobiles.  A solution M is prepared by mixingethanol and water. The mole fraction of ethanol in the mixture is 0.9.  Given Freezing point depression constant of water (K_(f)^(water)) = 1.86 K mol^(-1)  Freezing point depression constant of ethanol (K_(f)^(ethonal)) = 2.0 K kg mol^(-1)  Boiling point elevation constant of water (K_(b)^(water)) = 0.52 K kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethonal)) = 1.2 K kg mol^(-1)  Standard freezing point of water = 273 K  Standard freezing point of ethonal = 155.7 K  Standard boiling point of water = 373 K  Standard boiling point of ethanol = 351.5 K  Vapour pressure of pure water = 32.8 mm Hg  Vapour pressure of pure ethonal = 40 mm Hg  Molecular weight of water = 18 g mol^(-1)  Molecular weight of ethonal = 45 gmol^(-1)  In answering the following questions consider the solution to be ideal ideal solutions and solutes to be non-volatile and non-dissociative.  Water is added to the solution M such lthat the molecules fraction of water in t he solution becomes 0.9. The boiling point of this solution is

Accepted Answer

NA

Question 44

Properties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Application of colligative properties are very useful in day- to - day life. One of its examples is the use of ethylene glycol and water mixture as anti-freezing liquid in the radiator of automobiles.  A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9.  Given Freezing point depression constant of water (K_(f)^(water))=1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (e_(f)^(ethanol))=2.0 K kg mol^(-1)  Boiling point elevation constant of water (K_(b)^(water))=0.52 K kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol))=1.2 K kg mol^(-1)  Standard freezing point of water = 273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water = 373 K  Standard boiling point of ethanol = 351.5 K  Vapour pressure of pure water = 32.8 mm Hg  Vapour pressusre of pure ethanol = 40 mm Hg  Molecular weight of water = 18 g mol^(-1)  Molecular weight of ethanol = 46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative.  The vapour pressure of the solution M is

Accepted Answer

NA

Question 45

Properties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Application of colligative properties are very useful in day- to - day life. One of its examples is the use of ethylene glycol and water mixture as anti-freezing liquid in the radiator of automobiles.  A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9.  Given Freezing point depression constant of water (K_(f)^(water))=1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (e_(f)^(ethanol))=2.0 K kg mol^(-1)  Boiling point elevation constant of water (K_(b)^(water))=0.52 K kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol))=1.2 K kg mol^(-1)  Standard freezing point of water = 273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water = 373 K  Standard boiling point of ethanol = 351.5 K  Vapour pressure of pure water = 32.8 mm Hg  Vapour pressusre of pure ethanol = 40 mm Hg  Molecular weight of water = 18 g mol^(-1)  Molecular weight of ethanol = 46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative.  The freezing point of solution M is

Accepted Answer

NA

Question 46

Properties such as boiling point freezing point and vapour pressure of a pure solvent change Propeties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. One of its examples is the use of ethylene glycol and water mixtureas anti-freezing liquid in the radiator of automobiles. A solution M is prepared by mixing athanol and water. The mole fraction of ethanol in the mixture is 0.9  GivenFreezing point depression constant of water (K_(f)^(water))=1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (K_(f)^(ethanol))=2.0 K kg mol^(-1) Boiling point elevation constant of water (K_(b)^(water))=0.52 kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol))=1.2 kg mol^(-1)  Standard freezing point of water =273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water =373 K  tandard boiling point of ethanol =351.5 K  Vapour pressure of pure water =32.8 mmHg  Vapour presure of pure ethanol =40g Hg  Molecular weight of water =18 gmol^(-1)  Molecules weight of ethanol =46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative. when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. One of its examples is the use of ethylene glycol and water mixtureas anti-freezing liquid in the radiator of automobiles. A solution M is prepared by mixing athanol and water. The mole fraction of ethanol in the mixture is 0.9  GivenFreezing point depression constant of water (K_(f)^(water))=1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (K_(f)^(ethanol))=2.0 K kg mol^(-1) Boiling point elevation constant of water (K_(b)^(water))=0.52 kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol))=1.2 kg mol^(-1)  Standard freezing point of water =273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water =373 K  tandard boiling point of ethanol =351.5 K  Vapour pressure of pure water =32.8 mmHg  Vapour presure of pure ethanol =40g Hg  Molecular weight of water =18 gmol^(-1)  Molecules weight of ethanol =46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative. The freezing point of the solution M is

Accepted Answer

NA

Question 47

Properties such as boiling point freezing point and vapour pressure of a pure solvent change Propeties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. One of its examples is the use of ethylene glycol and water mixtureas anti-freezing liquid in the radiator of automobiles. A solution M is prepared by mixing athanol and water. The mole fraction of ethanol in the mixture is 0.9  GivenFreezing point depression constant of water (K_(f)^(water))=1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (K_(f)^(ethanol))=2.0 K kg mol^(-1) Boiling point elevation constant of water (K_(b)^(water))=0.52 kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol))=1.2 kg mol^(-1)  Standard freezing point of water =273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water =373 K  tandard boiling point of ethanol =351.5 K  Vapour pressure of pure water =32.8 mmHg  Vapour presure of pure ethanol =40g Hg  Molecular weight of water =18 gmol^(-1)  Molecules weight of ethanol =46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative. when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. One of its examples is the use of ethylene glycol and water mixtureas anti-freezing liquid in the radiator of automobiles. A solution M is prepared by mixing athanol and water. The mole fraction of ethanol in the mixture is 0.9  GivenFreezing point depression constant of water (K_(f)^(water))=1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (K_(f)^(ethanol))=2.0 K kg mol^(-1) Boiling point elevation constant of water (K_(b)^(water))=0.52 kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol))=1.2 kg mol^(-1)  Standard freezing point of water =273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water =373 K  tandard boiling point of ethanol =351.5 K  Vapour pressure of pure water =32.8 mmHg  Vapour presure of pure ethanol =40g Hg  Molecular weight of water =18 gmol^(-1)  Molecules weight of ethanol =46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative.Water is added to the solution M such that the fraction of water in the solution becomes 0.9. The boiling point of this solutions is

Accepted Answer

NA

Question 48

Properties such as boiling point freezing point and vapour pressure of a pure solvent change Propeties such as boiling point freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. One of its examples is the use of ethylene glycol and water mixtureas anti-freezing liquid in the radiator of automobiles. A solution M is prepared by mixing athanol and water. The mole fraction of ethanol in the mixture is 0.9  GivenFreezing point depression constant of water (K_(f)^(water))=1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (K_(f)^(ethanol))=2.0 K kg mol^(-1) Boiling point elevation constant of water (K_(b)^(water))=0.52 kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol))=1.2 kg mol^(-1)  Standard freezing point of water =273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water =373 K  tandard boiling point of ethanol =351.5 K  Vapour pressure of pure water =32.8 mmHg  Vapour presure of pure ethanol =40g Hg  Molecular weight of water =18 gmol^(-1)  Molecules weight of ethanol =46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative. when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-to-day life. One of its examples is the use of ethylene glycol and water mixtureas anti-freezing liquid in the radiator of automobiles. A solution M is prepared by mixing athanol and water. The mole fraction of ethanol in the mixture is 0.9  GivenFreezing point depression constant of water (K_(f)^(water))=1.86 K kg mol^(-1)  Freezing point depression constant of ethanol (K_(f)^(ethanol))=2.0 K kg mol^(-1) Boiling point elevation constant of water (K_(b)^(water))=0.52 kg mol^(-1)  Boiling point elevation constant of ethanol (K_(b)^(ethanol))=1.2 kg mol^(-1)  Standard freezing point of water =273 K  Standard freezing point of ethanol = 155.7 K  Standard boiling point of water =373 K  tandard boiling point of ethanol =351.5 K  Vapour pressure of pure water =32.8 mmHg  Vapour presure of pure ethanol =40g Hg  Molecular weight of water =18 gmol^(-1)  Molecules weight of ethanol =46 g mol^(-1)  In answering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative.The vapour pressure of the solution M is

Accepted Answer

NA

Question 49

Properties of elements X  (i) Its amide is used as a reducing agent  (ii) Its amalgam is used as reducing agent  Properties of element Y  (i) It is an octaatomic molecule  (ii) It is diamagnetic in ground state but paramagnetic in vapour phase  Properties of element Z  (i) Its diatomic molecule is paramagnetic  (ii) Its allotrope is an absorber of UV radiation  (iii) IT supports combustion  Which statement is not correct about these following compounds?

Accepted Answer

NA

Question 50

Properties of elements X  (i) Its amide is used as a reducing agent  (ii) Its amalgam is used as reducing agent  Properties of element Y  (i) It is an octaatomic molecule  (ii) It is diamagnetic in ground state but paramagnetic in vapour phase  Properties of element Z  (i) Its diatomic molecule is paramagnetic  (ii) Its allotrope is an absorber of UV radiation  (iii) IT supports combustion  Compound of XY and Z on reaction with Y form a compound A. Out of the following which statement is not correct about compoundA?

Accepted Answer

NA

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Propyne reacts with HOCl, which of the following cannot be formed

Propyne on polymerisation gives

Propyne to acetone

Propyne on oxidation with SeO_2 gives:

Propyne is formed by the reaction of

Propyne and propene can be distinguished by?

Propyne and propene can be distinguished by :

Propylene is passed through conc. H_2SO_4 and the product thus obtained on hydrolysis with boiling water gives

Propyl propionate is prepared from which of the following

Propyl iodide and isopropyl iodide are :

Propyl benzene reacts with bromine in the presence of light and heat to give :

Propose the mechanism of the reaction taking place when: (a). (-)-2-Bromooctane reacts with sodium hydroxide to form (+)-Octane-2-ol. (b). 2-Bromopentane is heated with KOH (alc). To form alkene.

Propose mechanism of the reaction taking place when (a) (-) - 2- Bromooctane reacts with sodium hydroxide to form (+) -octane -2-ol. (b) 2-Bromopentane is heated with (alc.) KOH to form alkenes.

Proportions because

Propiophenone is reduced by NaBH_(4) gives

Propionic acid with Br_(2)//P yields a dibromo product. Its structure would be

Propionic acid with Br_(2)//P yield a dibromo product . Its structure will be

Propionic acid with Br,/P yields a dibromo product. Its structure would be

Propionic acid is obtained from dry ice and what?

Propionic acid when treated with Br_(2) in the presence of P in sunlight gives :

Propionic acid on bromination in thepresence of red phosphorus gives 2- bromo propionic acids it shows

Propionic acid is subjected to reduction with hydroiodic acid in the presence of a little P, the product formed is

Propionic acid is obtainedby acidhydrolysis of

Propionic acid can also be named as

Propionic acid and KOH reacts to produce which one ofthe folliwng?

Propionamide when heated with amixture of bromine and caustic alkali wouldgive :

Propionaldoxime is reacted with trifluoroperoxy acetic acid gives

Propertyof alkaline earthmetals that increases with their atomic number is

Property of the alkali metals that increases with their atomic number is :

Property of the alkaline earth metals that increases with their atomic number is:

1.	Propyne reacts with HOCl, which of the following cannot be formed
Answer» `CH_(3)CH_(2)CHCl_(2)` `CH_(3)-OVERSET(O)overset(\|\|)(C)-CHCl_(2)` `{:(""CL),("\|"),(CH_(3)-CH-CHO):}` `{:(""O),("\|\|"),(ClCH_(2)-C-CH_(2)Cl):}` Solution : So, (a), (c) and (d) are correct ANSWERS while (b) is incorrect.

2.	Propyne on polymerisation gives
Answer» MESITYLENE BENZENE Ethyl benzene Propyl benzene Solution : Mesitylene or 1,3,5-trimethyl benzene

3.	Propyne to acetone
Answer» SOLUTION :Propyne to acetone : `UNDERSET("Propyne")(CH_(3)C=CH)+H_(2)Ounderset(1%HgSO_(4))OVERSET(40%H_(2)SO_(4))rarrunderset("alkenol")underset(OH)underset(\|)(CH_(3)-C=CH_(2))overset("tautomerisation")rarrunderset("acetone")underset(O)underset("\|\|")(CH_(3)-C-CH_(3))`

4.	Propyne on oxidation with SeO_2 gives:
Answer» CHOCHO `CH_3CH_2CHO` `CH_3COCHO` `CHOCH_2CHO` ANSWER :B

5.	Propyne is formed by the reaction of
Answer» `CH_3 Br` with sodium acetylide `CH_3I` with DISODIUM acetylide `CH_3I`with acetylene `CH_4` with chloroacetylene. Solution :`CH_3 Br + HC -= C Na to CH_3 - C -= CH + NaBr`

6.	Propyne and propene can be distinguished by?
Answer» conc. `H_(2)SO_(4)` `Br_(2)` in `C Cl_(4)` dil. `KMnO_(4)` `AgNO_(3)` in ammonia Answer :D

8.	Propylene is passed through conc. H_2SO_4 and the product thus obtained on hydrolysis with boiling water gives
Answer» 1-propanol 2-propanol 1-propanal 2-propanal. Solution :`CH_3 CH = CH_2 overset(H_2 SO_(4))(to) CH_3 - CH(OSO_(3) H)- CH_(3) overset(H_(2)O)UNDERSET("boil")(to) CH_(3) - CH OH - CH_(3)`

9.	Propyl propionate is prepared from which of the following
Answer» `CH_(3)CH_(2)CH_(2)OH,CH_(3)CH_(2)COOH` `CH_(3)COOH, CH_(3)(CH_(2))_(3)COOH` `CH_(3)CHOHCH_(3),CH_(3)CH_(2)COOH` `CH_(3)CH_(2)CH_(2)OH,(CH_(3))_(2)CHOOH` Solution :`CH_(3)CH_(2)CH_(2)OH+CH_(3)CH_(2)COOH overset(conc.H_(2)DSO_(4)) to UNDERSET("propyl propionate ")(CH_(3)CH_(2)COOCH_(2)CH_(2)CH_(3))`

10.	Propyl iodide and isopropyl iodide are :
Answer» FUNCTIONAL isomers Chain isomers Metamers Position isomers Answer :D

11.	Propyl benzene reacts with bromine in the presence of light and heat to give :
Answer» ANSWER :D

14.	Proportions because
Answer» of its acidic nature it is NEUTRAL it reacts with WATER it FORMS H - bonds Solution :`{:(.........H-O.........H-O.......),("\|\|"),(""C_(2)H_(5)"" H):}`

15.	Propiophenone is reduced by NaBH_(4) gives
Answer» 2-phenyl propan-2-ol 1-phenyl propan-1-ol 1-phenyl propan-2-ol 2-phenyl propan-1ol Answer :B

21.	Propionic acid on bromination in thepresence of red phosphorus gives 2- bromo propionic acids it shows
Answer» OPTICAL isomers tautomerism cis- trans isomers metamerism SOLUTION :`CH_(3) - CH_(2) - COOH + Br_(2) overset("Red P") to CH_(3)- CHBr - COOH` It SHOWS optical isomerism.

23.	Propionic acid is obtainedby acidhydrolysis of
Answer» `CH_(3) - CH_(2)-CH_(2)-NO_(2)` `CH_(3) - underset(CH_(3))underset(\|)overset(NO_(2))overset(\|)(CH)-CH_(3)` `CH_(3)-CH_(2)-CH_(2)_CN` `CH_(3) - underset(CH_(3))underset(\|)overset(CH_(3))overset(\|)(C) - NO_(2)` Solution :Primary nitroalkaneon acidhydrolysisgivesketone .

12.	Propose the mechanism of the reaction taking place when: (a). (-)-2-Bromooctane reacts with sodium hydroxide to form (+)-Octane-2-ol. (b). 2-Bromopentane is heated with KOH (alc). To form alkene.
Answer» Solution :(a). In this reaction, there is an inversion of configuration and `OH^(-)` ion (nucleophile) attacks from a side opposite to the side where Br atom is PRESENT. This means that the reaction FOLLOWS `S_(N^(1))` MECHANISM. (B). In this reaction bimolecular elimination (`E_(2)`-elimination) takes place. .

13.	Propose mechanism of the reaction taking place when (a) (-) - 2- Bromooctane reacts with sodium hydroxide to form (+) -octane -2-ol. (b) 2-Bromopentane is heated with (alc.) KOH to form alkenes.
Answer» SOLUTION :

16.	Propionic acid with Br_(2)//P yields a dibromo product. Its structure would be
Answer» `CHBr_(2)-CH_(2)COOH` `CH_(2)Br-CH_(2)-COBr` `CH_(3)-CBr_(2)-COOH` `CH_(2)Br-CHBR-COOH` Solution :Bromination occurs at `alpha`-position. `CH_(3)-overset(alpha)(C)H_(2)-COOH underset(-HBr)overset(Br_(2)//P)CH_(3)-CHBr-COOH underset(-HBr)overset(Br_(2)//P)toCH_(3)-CBr_(2)-COOH`

17.	Propionic acid with Br_(2)//P yield a dibromo product . Its structure will be
Answer» `H-UNDERSET(BR)underset(\|)overset(Br)overset(\|)(C)-CH_(2)COOH` `CH_(2)Br-CH_(2)COBr` `CH_(3)-underset(Br)underset(\|)overset(Br)overset(\|)(C)-COOH` `CH_(2)(Br)-CH(Br)-COOH` Solution :`CH_(3)CH_(2)COOHoverset(Br_(2)//P)toCH_(3)-underset(Br)underset(\|)overset(Br)overset(\|)(C)-COOH`

18.	Propionic acid with Br,/P yields a dibromo product. Its structure would be
Answer» `H - underset(Br)underset(\|)OVERSET(Br)overset(\|)C - CH_2COOH` `CH_3 - underset(Br) underset(\|)overset(Br)overset(\|)C - COOH` `CH_2 (Br) - CH_2 - COBr` `CH_2 (Br) - CH(Br) - COOH` ANSWER :B

19.	Propionic acid is obtained from dry ice and what?
Answer» `CH_(3)mgI` `C_(2)H_(5)MGBR` `C_(3)H_(7)MgBr` None of these Answer :B

20.	Propionic acid when treated with Br_(2) in the presence of P in sunlight gives :
Answer» `CH_(2)BrCH_(2)COOH` `CH_(3)CH_(2)COBR` `CH_(3)CHBrCOOH` `CH_(3)underset(Br"")underset(\|" ")(CH)COBr`, Answer :C

22.	Propionic acid is subjected to reduction with hydroiodic acid in the presence of a little P, the product formed is
Answer» Ethane Propane Butane None of these Solution :`underset"Propanoic ACID"(CH_3-CH_2-COOH+6HI)OVERSET"red P"to underset"Propane"(CH_3-CH_2-CH_3+2H_2O+3I_2`

24.	Propionic acid can also be named as
Answer» METHYL methanoic acid Methyl acetic acid Methyl ETHANOIC acid Ethyl acetic acid ANSWER :B

25.	Propionic acid and KOH reacts to produce which one ofthe folliwng?
Answer» Potassium propionate Propyl alcohol Propionaldehyde Does not react Solution :Propionic acid and KOH REACTS to produce potassium propionate. `UNDERSET("Propionic acid")(CH_(3)CH_(2)COOH)OVERSET(KOH)tounderset("Potassium propionate")(CH_(3)CH_(2)COOK+H_(2)O)`

26.	Propionamide when heated with amixture of bromine and caustic alkali wouldgive :
Answer» PROPYLAMINE PROPANOL PROPANAL ETHYLAMINE ANSWER :D

27.	Propionaldoxime is reacted with trifluoroperoxy acetic acid gives
Answer» propan-1-amine propan-2-amine 1-nitropropane 2-nitropropane ANSWER :C

28.	Propertyof alkaline earthmetals that increases with their atomic number is
Answer» IONISATION enthalpy Solubility of their hydroxides Solubility of their sulphates Electronegativity. Answer :B

29.	Property of the alkali metals that increases with their atomic number is :
Answer» Ionic molility of their ION in water Solubility of their sulphates Solubility of their carbonates Solubility of their hydroxides Solution :As SIZE of CATION increases, the size of hydrated ions in water DECREASES and thus ionic MOBILITY increases.

31.	Properties, whose values depend only on the concentration of solute particles in solution and not on the identity of the solute are called colligative properties.there may be change in number of moles of solute due to ionisation or association hence these properties are also affected.Number of moles of the product is related to degree of ionisation or association by van Hoff factor 'i' given by i=[1+(n-1)alpha] for dissociation where n is the number of products (ions or molecules ) obtained per mole of the reactant. & i=[1+(1/n-1)alpha] for association where n is number of reactant particles associated to give 1 mole product.A dilute solution contains 't' moles of solute X in 1 kg of solvent with molal elevation constant K_b.The solute dimerises in the solution according to the following equation.The degree of association is alpha. 2X hArr X_2 The equilibrium constant for the process can be expressed as
Answer» `K=(K_b t/(DeltaT_b))/(1-(K_bt)/(DeltaT_f))` `K=(K_b(K_bt-DeltaT_b))/([2DeltaT_b-K_bt]^2 `K=(2(K_(bt)-DeltaTb)//DeltaT_b)/(2t[1-(2(K_bt-DeltaT_b))/(DeltaT_b)])` `K=(DeltaT_("bobs"))/(DeltaT_("FOBS"))` Solution :`K=([X_2])/([X]^2)` , Here`{:(2X,hArr,X_2),(t, , 0):}` `1-talpha(talpha)/2{(DeltaT_b,=(1-alpha//2)K_bt),(alpha,=alpha=(2(K_bt-DeltaT_b))/(K_bt)):}` `implies [X_2]=talpha//2` `[X]=t-talpha` `K=(talpha//2)/((t-talpha)^2)=1/(2t^2)xxalpha/((1-alpha)^2)=1/(2t)xxalpha/((1-alpha)^2)=1/(2t)XX((2(K_bt-DeltaT_b))/(K_bt))/(1-((2(K_bt-DeltaT_b))/(K_bt))^2)` Hence , `K=(K_b(K_bt-DeltaT_b))/((2DeltaT_b-K_bt)^2)`

32.	Properties, whose values depend only on the concentration of solute particles in solution and not on the identity of the solute are called colligative properties.there may be change in number of moles of solute due to ionisation or association hence these properties are also affected.Number of moles of the product is related to degree of ionisation or association by van Hoff factor 'i' given by i=[1+(n-1)alpha] for dissociation where n is the number of products (ions or molecules ) obtained per mole of the reactant. & i=[1+(1/n-1)alpha] for association where n is number of reactant particles associated to give 1 mole product.A dilute solution contains 't' moles of solute X in 1 kg of solvent with molal elevation constant K_b.The solute dimerises in the solution according to the following equation.The degree of association is alpha. 2X hArr X_2 The colligaive properties observed will be
Answer» `{:(DeltaP_("THEO")gt,DeltaP_("actual")),(DeltaT_(b("theo"))gt,DeltaT_(b("actual"))),(DeltaT_(f("theo"))gt,DeltaT_(f("actual"))):}` `{:(DeltaP_("theo")=,DeltaP_("actual")),(DeltaT_(b("theo"))=,DeltaT_(b("actual"))),(DeltaT_(f("theo"))=,DeltaT_(f("actual"))):}` `{:(DeltaT_(b("theo"))lt,DeltaT_(b("actual"))),(DeltaT_(f("theo"))lt,DeltaT_(f("actual"))),(DeltaP_("theo")lt,DeltaP_("actual")):}` `{:(DeltaP_("theo")GE,DeltaP_("actual")),(DeltaT_(b("theo"))=,DeltaT_(b("actual"))),(DeltaT_(f("theo"))lt,DeltaT_(f("actual"))):}` SOLUTION :During association `DeltaP_(theo)gt DeltaP_("actual"),DeltaT_(b"theo"))gt DeltaT_(b("actual")),DeltaT_("theo")gt DeltaT_("actual")`

33.	Properties such as boiling point, freezing point and vapour pressure of a pure solvent change when solute molecules are added to homegenous solution. These are called colligative properties. Applications of colligative properties are very useful in day to day life. One of its exaples is the use of ethylene glycol and water mixtue as anti-freezing liquid in the radiators of automobiles. A solution M is prepared by mixing ehanol and water. The mole fraction of ethanol in the mixture is 0.9 Given. K_(f)"of water"=1.86 "K kg mol"^(-1) K_(f)"of ethanol" = 2.0 "K kg mol"^(-1) K_(b)"for water "=0.52 "K kg mol"^(-1) K_(b)" of ethanol"=1.2 "K kg mol"^(-1) T_(f)("water")=273 K T_(f)("ethanol")=155.7 K T_(b)^(@) ("water")=373 K T_(b)^(@)("ethanol")=351.5 K P^(@)("water")32.8 mm Hg. P^(@)("ethanol")=40 mmHg M("ethanol")==46 "g mol"^(-1) M("water")=18"g mol"^(-1) In answering the following quesion, consider the solutions to be ideal dilute solutions ans solute to be non-voltile and non-dissoviative. (7) water is added to the solution M such that the mole fraction so wter in solution becomes 0.9. The boiling point of solution is :
Answer» `380.4 K` `376.2 K` 357.5 K` 245.7 K` SOLUTION :In this case, water is solvent and ETHANOL is SOLUTE `"Molality of solution (m)"=("No. of MOLES ethanol")/("Mass of water in kg")` `n_("ethanol")=0.1 `, `W_("water")=((0.9mol)xx(18" g mol"^(-1)))/1000=0.0162 kg.` `m=((0.1mol))/((0.0162 kg))=6.173 "mol kg"^(-1)` =6.173m `DeltaT_(b)=K_(b)xxm=(0.52"k kg mol"^(-1))xx(6.173" mol kg"^(-1))=3.2 K` b.p. of solution = 373+3.2= 376.2 K

34.	Properties such as boiling point, freezing point and vapour pressure of a pure solvent change when solute molecules are added to homegenous solution. These are called colligative properties. Applications of colligative properties are very useful in day to day life. One of its exaples is the use of ethylene glycol and water mixtue as anti-freezing liquid in the radiators of automobiles. A solution M is prepared by mixing ehanol and water. The mole fraction of ethanol in the mixture is 0.9 Given. K_(f)"of water"=1.86 "K kg mol"^(-1) K_(f)"of ethanol" = 2.0 "K kg mol"^(-1) K_(b)"for water "=0.52 "K kg mol"^(-1) K_(b)" of ethanol"=1.2 "K kg mol"^(-1) T_(f)("water")=273 K T_(f)("ethanol")=155.7 K T_(b)^(@) ("water")=373 K T_(b)^(@)("ethanol")=351.5 K P^(@)("water")32.8 mm Hg. P^(@)("ethanol")=40 mmHg M("ethanol")==46 "g mol"^(-1) M("water")=18"g mol"^(-1) In answering the following quesion, consider the solutions to be ideal dilute solutions ans solute to be non-voltile and non-dissoviative. (5) The freezing point of solution M is:
Answer» `268.7 K` `268.5 K` `234.5 K` `150.9 K` Solution :MOLALITY of solution (m) `=("No. of MOLES of WATER")/("Mass of ethanol in kg")` `n_("ethanol")=0.1 mol` `W_("ethnol")=((0.9"mol"))/((0.0414 kg))=2.415 " mol kg"^(-1)` =2.415 m. `DeltaT_(f)=K_(f)xxm=(2.0" K kg mol mol"^(-1))XX(2.415 "mol kg"^(-1))=4.83 K.` f.p. of solution =155.7-4.83=150.87 K.

35.	Properties such as boiling point, freezing point and vapour pressure of a pure solvent change when solute molecules are added to homegenous solution. These are called colligative properties. Applications of colligative properties are very useful in day to day life. One of its exaples is the use of ethylene glycol and water mixtue as anti-freezing liquid in the radiators of automobiles. A solution M is prepared by mixing ehanol and water. The mole fraction of ethanol in the mixture is 0.9 Given. K_(f)"of water"=1.86 "K kg mol"^(-1) K_(f)"of ethanol" = 2.0 "K kg mol"^(-1) K_(b)"for water "=0.52 "K kg mol"^(-1) K_(b)" of ethanol"=1.2 "K kg mol"^(-1) T_(f)("water")=273 K T_(f)("ethanol")=155.7 K T_(b)^(@) ("water")=373 K T_(b)^(@)("ethanol")=351.5 K P^(@)("water")32.8 mm Hg. P^(@)("ethanol")=40 mmHg M("ethanol")==46 "g mol"^(-1) M("water")=18"g mol"^(-1) In answering the following quesion, consider the solutions to be ideal dilute solutions ans solute to be non-voltile and non-dissoviative. (6) The vapour pressure of solution M is :
Answer» <P>`39.3 MM Hg` `36.0 mm Hg` `25.2 mm Hg` `28.8 mm Hg` Solution :V.P. of solution (p) =`P_(A)^(@)X_(A)` =(40 mm Hg)xx(0.9)=36 mm Hg

36.	A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9 Given: Freezing point depression constant of water (K_(f)^(water)=1.86 K kg mol^(-1)) Freezing point depression constant to ethanol (K_(f)^(ethanol))=2.0 K kg mol^(-1)) Boiling point elevation constant of water (K_(b)^(water))=0.52 K kg mol^(-1)) Boiling point elevation constant of ethanol (K_(b)^(ethanol))=1.2 K kg mol^(-1)) Standard freezing point of water = 273 K Standard freezing point of ethanol = 155.7 K Standard boilingpoint of water = 373 K Standard boilingpoint of ethanol = 351.5 K Vapour pressure of pure water =32.8 mm Hg Vapour pressure of pure ethanol =40 mm Hg Molecular weight of water =18 g mol^(-1) Molecular weight of ethanol =46 g mol^(-1) In anwering the following questions consider the solutions to be ideal dilute solutions and solutes to be non-volatile and non-dissociative. Water is added to the solution M such that the mole fraction of water in the solution becomes 0.9. The boiling point of this solution is
Answer» `380.4 K` `376.2 K` `375.5K` `354.7K` SOLUTION :`x_(H_(2)O)=0.9("solvent"),x_(C_(2)H_(5)OH)=0.1("solute")` `DeltaT_(B)=K_(b)xxm` `=0.52xx(0.1xx1000)/(0.9xx18)=3.2K` `:.`Boiling point, `T_(b)=(373+3.2)K` `=376.2K`