Ramendra C Mukerjee Solutions for Chapter: Miscellaneous Objective Questions, Exercise 1: Exercise 1

In an electrolysis process, $10$ electrons could deposit $x \mathrm{kg}$ of a univalent metal $\mathrm{M}$. The atomic weight of $\mathrm{M}$ is ($\mathrm{N}$ is Avogadro constant.)

Which of the following compound cannot be oxidised by ${\mathrm{O}}_3$?

In which of the following compounds the cations are present in alternate tetrahedral voids

The elevation in boiling point of a solution of $13.44 \mathrm{g}$ of ${\mathrm{CuCl}}_2$ in $1 \mathrm{kg}$ of water using the following information, will be (Molecular weight of ${\mathrm{CuCl}}_2=134.4$ and ${\mathrm{K}}_{\mathrm{b}}=0.52 \mathrm{K} {\mathrm{molal}}^{-1}$) : (Report the answer in two decimal places)

Which of the following choices match(es) with hydrogen gas at $200 \mathrm{atm}$ and $273 \mathrm{K}$?

A solution $\mathrm{M}$ is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is $0.9$. 

Given,

$\begin{array}{l}{\mathrm{K}}_{\mathrm{f}} \left(\mathrm{water}\right)=1.86 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}\\ {\mathrm{K}}_{\mathrm{f}} \left(\mathrm{ethanol}\right)=2.0 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}\\ {\mathrm{K}}_{\mathrm{b}} \left(\mathrm{water}\right)=0.52 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}\\ {\mathrm{K}}_{\mathrm{b}} \left(\mathrm{ethanol}\right)=1.2 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}\end{array}$

Standard freezing point of water $=273 \mathrm{K}$

Standard freezing point of ethanol $=155.7 \mathrm{K}$

Standard boiling point of water $=373 \mathrm{K}$

Standard boiling point of ethanol $=351.5 \mathrm{K}$

Vapour pressure of pure water $=32.8 \mathrm{mmHg}$ 

Vapour pressure of pure ethanol $=40 \mathrm{mmHg}$ 

Molecular weight of water $=18 \mathrm{g} {\mathrm{mol}}^{-1}$

Molecular weight of ethanol $=46 \mathrm{g} {\mathrm{mol}}^{-1}$

The vapour pressure of the solution $\mathrm{M}$ is

A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is $0.9 .$ Given

$\begin{array}{l}{\mathrm{K}}_{\mathrm{f}}\left(\mathrm{Water}\right)=1.86 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}\\ {\mathrm{K}}_{\mathrm{f}}\left(\mathrm{Ethanol}\right)=2.0 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}\\ {\mathrm{K}}_{\mathrm{b}}\left(\mathrm{Water}\right)=0.52 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}\\ {\mathrm{K}}_{\mathrm{b}}\left(\mathrm{Ethanol}\right)=1.2 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}\end{array}$

Standard freezing point of water $=273\mathrm{K}$

Standard freezing point of ethanol $=155.7 \mathrm{K}$

Standard boiling point of water $=373 \mathrm{K}$

Standard boiling point of ethanol $=351.5 \mathrm{K}$

Vapour pressure of pure water $=32.8 \mathrm{mmHg}$ 

Vapour pressure of pure ethanol $=40 \mathrm{mmHg}$ 

Molecular weight of water $=18 \mathrm{g} {\mathrm{mol}}^{-1}$

Molecular weight of ethanol$=46 \mathrm{g} {\mathrm{mol}}^{-1}$ 

Water is added to the solution M such that the mole fraction of water in solution becomes 0.9. What is the boiling point of this solution?

[Hint: Solute is ethanol and solvent is water]

The solubility product $\left({\mathrm{K}}_{\mathrm{sp}}\right)$ of salts of types $\mathrm{MX}, {\mathrm{MX}}_2$ and ${\mathrm{M}}_3\mathrm{X}$ at a temperature ${}^{\text{'}}\mathrm{T}^{\text{'}}$ are $4.0\times {10}^{-8},3.2\times {10}^{-14}$ and $2.7\times {10}^{-15}$ respectively. Solubilities $\left(\mathrm{mol} {\mathrm{dm}}^{-3}\right)$ of salts at temperature $\text{'}$$\mathrm{T}$$\text{'}$ are in the order: