Embibe Experts Solutions for Chapter: Equilibrium, Exercise 4: Exercise 4

On adding $0.1 \mathrm{M}$ solution each of $\left[{\mathrm{Ag}}^{+}\right], \left[{\mathrm{Ba}}^{2+}\right], \left[{\mathrm{Ca}}^{2+}\right]$ in a ${\mathrm{Na}}_2{\mathrm{SO}}_4$ solution, species first precipitated is

$\left[{\mathrm{K}}_{\mathrm{sp}}{\mathrm{BaSO}}_4={10}^{-11}, {\mathrm{K}}_{\mathrm{sp}}{\mathrm{CaSO}}_4={10}^{-6}, {\mathrm{K}}_{\mathrm{sp}}{\mathrm{Ag}}_2{\mathrm{SO}}_4={10}^{-5}\right]$

The reaction quotient $\left(\mathrm{Q}\right)$ for the reaction; ${\mathrm{N}}_{2( \mathrm{g})}+3{\mathrm{H}}_{2( \mathrm{g})}\rightleftharpoons 2{\mathrm{NH}}_{3( \mathrm{g})}$ is given by $\mathrm{Q}=\frac{{\left[{\mathrm{NH}}_3\right]}^2}{\left[ {\mathrm{N}}_2\right]{\left[{\mathrm{H}}_2\right]}^3}.$ The reaction will proceed from right to left if :-

The values of ${\mathrm{K}}_{{\mathrm{P}}_1}$ and ${\mathrm{K}}_{{\mathrm{P}}_2}$ for the reactions $\mathrm{X}\rightleftharpoons \mathrm{Y}+\mathrm{Z}$ ........(1) and $\mathrm{A}\rightleftharpoons 2\mathrm{B}$ .......(2) are in the ratio $9:1$. If degree of dissociation of $\mathrm{X}$ and $\mathrm{A}$ be equal, then total pressure at equilibrium $\left(1\right)$ and $\left(2\right)$ are in the ratio:

The reaction,

$2 \mathrm{A}\left(\mathrm{g}\right)+\mathrm{B}\left(\mathrm{g}\right)\rightleftharpoons 3\mathrm{C}\left(\mathrm{g}\right)+\mathrm{D}\left(\mathrm{g}\right)$

is begun with the concentrations of $\mathrm{A}$ and $\mathrm{B}$ both at an initial value of $1.00 \mathrm{M}.$ When equilibrium is reached, the concentration of $\mathrm{D}$ is measured and found to be $0.25 \mathrm{M}.$ The value for the equilibrium constant for this reaction is given by the expression:

The equilibrium constants ${\mathrm{K}}_{{\mathrm{P}}_1}$ and ${\mathrm{K}}_{{\mathrm{P}}_2}$ for the reactions $\mathrm{X}\rightleftharpoons 2\mathrm{Y}$ and $\mathrm{Z}\rightleftharpoons \mathrm{P}+\mathrm{Q}$, respectively are in the ratio of $1:9$. If the degree of dissociation of $\mathrm{X}$ and $\mathrm{Z}$ be equal then the ratio of total pressures at these equilibria is

The value of ${\mathrm{K}}_{\mathrm{p}}/{\mathrm{K}}_{\mathrm{C}}$ for the following reactions at $300 \mathrm{K}$ are, respectively (At $300\mathrm{K}, \mathrm{RT}=24.62 {\mathrm{dm}}^3 \mathrm{atm} {\mathrm{mol}}^{-1}$)

${\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)$

${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$

In a chemical reaction, $\mathrm{A}+2\mathrm{B}\stackrel{\mathrm{k}}{\rightleftharpoons }2\mathrm{C}+\mathrm{D},$ the initial concentration of $\mathrm{B}$ was $1.5$ times of the concentration of $\mathrm{A},$ but the equilibrium concentrations of $\mathrm{A}$ and $\mathrm{B}$ were found to be equal. The equilibrium constant $\left(\mathrm{K}\right)$ for the aforesaid chemical reaction is

Two solids dissociate as follows

$\mathrm{A}\left(\mathrm{s}\right)=\mathrm{B}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{g}\right); {\mathrm{K}}_{{\mathrm{p}}_1}=\mathrm{x}.{\mathrm{atm}}^2$

$\mathrm{D}\left(\mathrm{s}\right)=\mathrm{C}\left(\mathrm{g}\right)+\mathrm{E}\left(\mathrm{g}\right); {\mathrm{K}}_{\mathrm{p}2}=\mathrm{y}·{\mathrm{atm}}^2$

The total pressure when both the solids dissociate simultaneously is :