S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: Equilibrium in Physical and Chemical Processes, Exercise 20: PROBLEMS FOR PRACTICE

In an experiment, $2$ moles of $\mathrm{HI}$ are taken into an evacuated $10.0$ litre container at $720 \mathrm{K}$. The equilibrium constant equals to $0.0156$ for the gaseous reaction, $2\mathrm{HI}\left(\mathrm{g}\right) \rightleftharpoons {\mathrm{H}}_{2(}\mathrm{g})+{\mathrm{I}}_2(\mathrm{g})$. Calculate the amounts of $\mathrm{HI}\left(\mathrm{g}\right)$,${\mathrm{H}}_2\left(\mathrm{g}\right)$,${\mathrm{I}}_2\left(\mathrm{g}\right)$ at equilibrium.

When ${\mathrm{PCl}}_5$ is heated in a closed vessel at $575 \mathrm{K}$, the total pressure at equilibrium is found to be $1 \mathrm{atm}$ and partial pressure of ${\mathrm{Cl}}_2$ is found to the $0.324$ atm. Calculate the equilibrium constant (${\mathrm{K}}_{\mathrm{p}}$) for the decomposition reaction.

A reaction mixture containing ${\mathrm{N}}_2$ at $0.50 \mathrm{atm}$, ${\mathrm{H}}_2$ at $3.0 \mathrm{atm}$ and ${\mathrm{NH}}_3$ at $0.50 \mathrm{atm}$ is heated to ${450}^{° }\mathrm{C}$. In which direction the reaction ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\stackrel{ }{\rightleftharpoons }2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ will go if ${\mathrm{K}}_{\mathrm{p}}$ is $4.28\times {10}^{-5}$?

The equilibrium constant for the reaction ${\mathrm{CH}}_3\mathrm{COOH}+{\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}\stackrel{ }{\rightleftharpoons }{\mathrm{CH}}_3{\mathrm{COOC}}_2{\mathrm{H}}_5+{\mathrm{H}}_2\mathrm{O}$ is $4.0$ at ${25}^{°} \mathrm{C}$. Calculate the weight of ethyl acetate that will be obtained when $120 \mathrm{g}$ of acetic acid are reacted with $92 \mathrm{g}$ of alcohol.

At ${448}^{°} \mathrm{C}$, the equilibrium constant (${\mathrm{K}}_{\mathrm{c}}$) for the reaction, ${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)\stackrel{ }{\rightleftharpoons }2\mathrm{HI}\left(\mathrm{g}\right)$, is $50.5$. Predict the direction in which the reaction will proceed to reach equilibrium at ${448}^{°} \mathrm{C}$, if we start with $2.0\times {10}^{-2} \mathrm{mol}$ of $\mathrm{HI}$, $1.0\times {10}^{-2} \mathrm{mol}$ of ${\mathrm{H}}_2$ and $3\times {10}^{-2} \mathrm{mol}$ of ${\mathrm{I}}_2$ in a $2.0 \mathrm{L}$ container.

For the reaction, $2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)\stackrel{ }{\rightleftharpoons }2\mathrm{NOCl}\left(\mathrm{g}\right)$, if partial pressure ${\mathrm{p}}_{\mathrm{NOCl}}=0.32 \mathrm{atm}$, ${\mathrm{p}}_{\mathrm{NO}}=0.22 \mathrm{atm}$ and ${\mathrm{p}}_{{\mathrm{Cl}}_2}=0.11 \mathrm{atm}$, then find ${\mathrm{K}}_{\mathrm{p}}$.

The ${\mathrm{K}}_{\mathrm{p}}$ value for reaction ${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)\stackrel{ }{\rightleftharpoons }2\mathrm{HI}\left(\mathrm{g}\right)$ at ${460}^{°} \mathrm{C}$ $49$. If the initial pressure of ${\mathrm{H}}_2$ and ${\mathrm{I}}_2$ is $0.5 \mathrm{atm}$ respectively, determine the partial pressure of each gas at equilibrium.

The reaction ${\mathrm{CH}}_3\mathrm{COOH}\left(\mathrm{l}\right)+{\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}\left(\mathrm{l}\right)\stackrel{ }{\rightleftharpoons }{\mathrm{CH}}_3{\mathrm{COOC}}_2{\mathrm{H}}_5\left(\mathrm{l}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$ was carried out at ${27}^{°} \mathrm{C}$ by taking one mole of each of the reactants. The reaction reached equilibrium when $\frac{2}{3}$rd of the reactants were consumed. Calculate the free energy change for the reaction ($\mathrm{R}=8.314 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$).