Chemical and Ionic Equilibrium 1 Question 18
19. At constant temperature, the equilibrium constant $\left(K_{p}\right)$ for the decomposition reaction, $\mathrm{N}{2} \mathrm{O}{4} \rightleftharpoons 2 \mathrm{NO}{2}$, is expressed by $K{p}=\frac{4 x^{2} p}{\left(1-x^{2}\right)}$, where, $p=$ pressure, $x=$ extent of decomposition. Which one of the following statement is true?
(2001, 1M)
(a) $K_{p}$ increases with increase of $p$
(b) $K_{p}$ increases with increase of $x$
(c) $K_{p}$ increases with decrease of $x$
(d) $K_{p}$ remains constant with change in $p$ and $x$
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Solution:
- $\underset{1-x}{\mathrm{~N}{2} \mathrm{O}{4}} \rightleftharpoons \underset{2 x}{2 \mathrm{NO}{2}}, K{p}=\frac{4 x^{2} p}{1-x^{2}} \cdot K_{p}$ is function of temperature only, does not change with either $p$ or $x$.
