Seema Saini Solutions for Chapter: Chemical Equilibrium, Exercise 2: DPP 6.2

The value of ${\mathrm{K}}_{\mathrm{p}}$ for the reaction, $2{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)+2{\mathrm{Cl}}_2 \left(\mathrm{g}\right)\rightleftharpoons 4\mathrm{HCl} \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)$, is $0.03 \mathrm{atm}$ at $427 °\mathrm{C}$.

 When the partial pressure is expressed in $\mathrm{atm}$, the value of ${\mathrm{K}}_{\mathrm{C}}$ for the same reaction is 

The equilibrium constant of the reaction ${\mathrm{SO}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{SO}}_3\left(\mathrm{g}\right)$ is $4\times {10}^{-3}$. The equilibrium constant of the reaction $2{\mathrm{SO}}_3\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$ would be

The equilibrium constant for $2{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{S}}_2\left(\mathrm{g}\right)$ is $0.0118$ at $1300 \mathrm{K}$, while the heat of dissociation is $597.4 \mathrm{kJ}$. The standard equilibrium constant of the reaction at $1200\mathrm{K}$ is

When ethanol and acetic acid were mixed together in an equimolar proportion, $66.6\%$ is converted into ethyl acetate. Calculate ${\mathrm{K}}_{\mathrm{C}}$. Also, calculate the quantity of ester produced, if one mole of acetic acid is treated with $0.5 \mathrm{mol}$ and $4 \mathrm{mol}$ of alcohol, respectively.

In an aqueous solution of volume $500 \mathrm{mL}$, when the reaction of $2{\mathrm{Ag}}^{+}+\mathrm{Cu}\rightleftharpoons {\mathrm{Cu}}^{2+}+2\mathrm{Ag}$ has reached the equilibrium, $\left[{\mathrm{Cu}}^{2+}\right]$ was $\mathrm{x} \mathrm{M}$. When $500 \mathrm{mL}$ of water is further added at equilibrium, $\left[{\mathrm{Cu}}^{2+}\right]$ will be

Consider following reactions in equilibrium concentration $0.01 \mathrm{M}$ of every species.
$\left(\mathrm{I}\right) {{\mathrm{PCl}}_5}_{\left(\mathrm{g}\right)}\rightleftharpoons {{{\mathrm{PCl}}_3}_{(\mathrm{g}}}_{)}+{{\mathrm{Cl}}_2}_{\left(\mathrm{g}\right)}$
$\left(\mathrm{II}\right) 2{\mathrm{HI}}_{\left(\mathrm{g}\right)}\rightleftharpoons {{\mathrm{H}}_2}_{\left(\mathrm{g}\right)}+{{\mathrm{I}}_2}_{\left(\mathrm{g}\right)}$
$\left(\mathrm{III}\right) {{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+3{{\mathrm{H}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons 2{{\mathrm{NH}}_3}_{\left(\mathrm{g}\right)}$
The extent of the reactions taking place is

A reaction ${\mathrm{S}}_8\left(\mathrm{g}\right)\rightleftharpoons 4{\mathrm{S}}_2\left(\mathrm{g}\right)$ is carried out by taking $2 \mathrm{moles}$ of ${\mathrm{S}}_8\left(\mathrm{g}\right)$ and $0.2 \mathrm{mole}$ of ${\mathrm{S}}_2\left(\mathrm{g}\right)$ in a reaction vessel of $1 \mathrm{litre}$ at $900 \mathrm{K}$. Which are correct if ${\mathrm{K}}_{\mathrm{C}}=6.30\times {10}^{-6} ?$

(a) ${{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+{{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons 2{\mathrm{NO}}_{\left(\mathrm{g}\right)}; {\mathrm{K}}_1$
(b) $\left(\frac{1}{2}\right){{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+\left(\frac{1}{2}\right){{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons \mathrm{NO}\left(\mathrm{g}\right); {\mathrm{K}}_2$
(c) $2{{\mathrm{NO}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons {{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+{{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}; {\mathrm{K}}_3$
(d) ${\mathrm{NO}}_{\left(\mathrm{g}\right)}\rightleftharpoons \left(\frac{1}{2}\right){{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+\left(\frac{1}{2}\right){{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}; {\mathrm{K}}_4$

The correct relation between ${\mathrm{K}}_1, {\mathrm{K}}_2, {\mathrm{K}}_3$ and ${\mathrm{K}}_4$ is/are