Question 73. For the reaction {\mathrm N}_2{\mathrm O}_4(\mathrm g)\rightleftharpoons2{\mathrm{NO}}_2(\mathrm g), \mathrm{K}{\mathrm{p}}=0.492 atm at 300 K. The value of \mathrm{K}_{\mathrm{c}} for the reaction at the same temperature is ____ \times10^{-2}.
(Given: \mathrm{R}=0.082 L atm mol⁻¹ K⁻¹)
Answer: (2)
Explanation:
The relation between \mathrm{K}{\mathrm{p}} and
\mathrm{K}{\mathrm{c}} is
\mathrm{K}{\mathrm{p}}=\mathrm{K}{\mathrm{c}}(\mathrm{R}\mathrm{T})^{\Delta \mathrm{n}_{\mathrm{g}}}For the given reaction, \Delta \mathrm{n}_{\mathrm{g}}=2-1=1.
Substituting the values,
\mathrm{K}{\mathrm{c}}=\frac{\mathrm{K}{\mathrm{p}}}{\mathrm{R}\mathrm{T}}\mathrm{K}_{\mathrm{c}}=\frac{0.492}{0.082\times300}.
On calculation, \mathrm{K}_{\mathrm{c}}=2\times10^{-2}.