Elevation in Boiling Point

Q. what is the sequence of boiling point of alcohol, aldehyde, ketone, ether, carboxylic acid, amine and amide with proper reason?

Q. Molarity of 29%(w/w) H2SO4 solution whose density is 1.22 g/ml, is ?

Q. The solution is prepared by mixing $8.5g$ of $C{H}_{2}C{l}_2$ and $11.95g$ of $CHC{l}_3$ at $298K$ are $415$ and $200mmHg$ respectively, the mole fraction of $CHC{l}_3$ in vapour form is: (Molar mass of $Cl=35.5gmo{l}^{-1}$)
(JEE Main - 2017)

1. $0.325$
2. $0.486$
3. $0.162$
4. $0.675$

Q. The compound with the highest boiling point is Propanal Propanone Acetic acid Propan 1 ol

Q. 1.1 mole of A is mixed with 1.2 mol of B and themixture is kept in a 1 L flask till the equilibriumA+2B 2C+D is reached. At equilibrium0.1 mol of D is formed. The K of the reaction(1) 0.002(2) 0.004(3) 0.001(4) 0.003

Q.

0.1 M NaCl and 0.1 M CH₃COOH are kept in separate containers. If their osmotic pressures Are P₁ and P₂ respectively then the correct statement is:

1. P₁> P₂

2. P₁= P₂

3. P₁< P₂

4. P₁= P₂ = 0 atm

Q.

The rise in the boiling point of a solution containing 1.8 gram of glucose in 100g of a solvent in 0.1⁰C. The molal elevation constant of the liquid is

1. 0.01 K/m

2. 0.1 k/m

3. 1 K/m

4. 10 K/m

Q. If the density of a certain gas at 30 degree C and 768 torr is 1.35 kg/m3 its density at STP would be 1. 1.48 kg/m3 2. 1.58 kg/m3 3. 1.25 kg/m3 4. 1.4 kg/m3

Q.

Which one of the following aqueous solutions will exhibit highest boiling point?

1. 0.015 M urea

2. 0.01 M KNO₃

3. 0.01 M Na₂SO₄

4. 0.015 M glucose

Q. Which of the following having higher boiling point 1 propanal Acetone Ethanol Propane

Q.

Which one of the following would produce maximum elevation in boiling point?

1. 0.1 M glucose

2. 0.2 M glucose

3. 0.1 M barium chloride

4. 0.1 M magnesium sulphate

Q.

If 0.15g of a solute dissolved in 15g of solvent is boiled at a temperature higher by 0.216⁰C than that of the pure solvent, then the molecular weight of the

substance is (molal elevation constant for the solvent is 2.16):

1. 1.01

2. 10

3. 10.1

4. 100

Q. which of the following molecule is polar 1] PF3Cl2 2] PCl5 3] PCl3F2 4] XeF4

Q. Equal masses of H_{2 }O_2 and Methane have been taken in a container of volume V at temperature 27 degree celsius in identical conditions the ratio of the volume of the gases H_{2 }:O_2:Methane would be

Q.

A 0.2 molal aqueous solution of a weak acid (HX) is 20% ionised. The freezing point of this solution is (Given for water)

1. - 0.31° C

2. - 0.45°C

3. - 0.53°C

4. - 0.90°C

Q.

Which of the following statements is correct for the boiling point of solvent containing a dissolved solid substance

1. Boiling point of the liquid is depressed
2. Boiling point of the liquid is elevated
3. There is no effect on the boiling point
4. The change depends upon the polarity of liquid

Q.

The boiling point of benzene is 353.23 K. When 1.80 g of a non-volatile solute was dissolved in 90 g benzene, the boiling point is raised to 354.11 K. Calculate the molar mass of the solute. $\left(K_{b}forbenzeneis2.53Kkgmo{l}^{-1}\right)$

1. $58.0gmo{l}^{-1}$

2. $68.0gmo{l}^{-1}$

3. $78.0gmo{l}^{-1}$

4. $48.0gmo{l}^{-1}$

Q. 14. For whose ionisation , equilibrium constant is highest ? 1. HI 2.HBr 3.HCl 4.HF

Q. What would be the concentration of Cl- ions when equal volumes of aqueous solutions of 0.01M NH4Cl and 0.02M Al2(SO4)3 , are mixed ? (1) 0.005 (2) 0.01 (3) 0.001 (4) 0.05

Q.

The boiling point of a solution of 0.105 gm of a substance in 15.84 gram of ether was found to be 100°C higher than that of pure ether. What is the molecular weight of the substance [Molecular elevation constant of ether per 100 g = 21.6]

1. 144.50

2. 143.18

3. 140.28

4. 146.66

Q.

18g of glucose $\left(C_6{H}_{12}{O}_6\right)$ is dissolved in 1 kg of water in a saucepan. At what temperature will the water boil (at 1 atm)? $K_b$ for water is $0.52Kkgmo{l}^{-1}$.

1. 373.202K

2. 365.202K

3. 370.202K

4. 473.202K

Q.

Normal boiling point of water is 373 K (at 760mm). Vapour pressure of water at 298 K is 23 mm. If the enthalpy of evaporation is 40.656 kJ/mole, the boiling point of water at 23 mm pressure will be

1. 250 K

2. 294 K

3. 51.6 K

4. 12.5 K

Q. Is this formula always applicable, α x molarity = concentration of ions in solution? (α is degree of dissociation)

Q. In a 0.2 molal aqueous solution of a weak acid HX, the degree of ionization is 0.3 at room temperature. Taking $K_f$ for water as $1.85{}^{o}C{m}^{-1}$, the freezing point of the solution will be nearest to

1. $-0.481{}^{\circ }C$
2. $-0.360{}^{\circ }C$
3. $-0.260{}^{\circ }C$
4. $-0.150{}^{\circ }C$

Q. Mass of $112ml$ of oxygen at NTP on liquefaction would be:

1. $0.32$
2. $0.64g$
3. $0.96g$
4. $0.16g$

Q.

A 0.001 molal solution of in water had a freezing point depression of 0.0054°C. If K_f for water is 1.80, the correct formulation for the above molecule is

1. 

2. 

3. 

4. 

Q.

0.1 M NaCl and 0.1 M CH₃COOH are kept in separate containers. If their osmotic pressures Are P₁ and P₂ respectively then the correct statement is:

1. P₁> P₂

2. P₁= P₂

3. P₁< P₂

4. P₁= P₂ = 0 atm

Q. Calculate the value of ebullioscopic constant of a solvent if enthalpy of vapourisation of that solvent is nearly $3974calmo{l}^{-1}$.
Given :
Boiling point of pure solvent is ${127}^{\circ }C$
Molecular mass of the solvent is $20gmo{l}^{-1}$

1. $2.4Kkgmo{l}^{-1}$
2. $0.5Kkgmo{l}^{-1}$
3. $1.6Kkgmo{l}^{-1}$
4. $3.2Kkgmo{l}^{-1}$

Q. 10 mL of C2H4 (g) is exploded with O2 (excess). The contraction in volume will be

Q. 49.Two identical flasks x and y contain 64g of methane and 100 g of an unknown gas A2 resp at 2 atm and 300k . The vapour density of gas A2 will be