Question

At $1000\, K$, the equilibrium constant. $K_{C}$ for the reaction $2 NOCl (g) \rightleftharpoons 2 NO (g)+ Cl _{2}(g)$ is $4.0 \times 10^{-6} mol\, L ^{-1}$. The $K_{P}$ (in bar) at the same temperature is $\left(R=0.083 \,L\right.$ bar $\left. K ^{-1}\, mol ^{-1}\right)$

• A. $3.32 \times 10^{-6}$
• B. $3.32 \times 10^{4}$
• C. $3.32 \times 10^{-4}$
• D. $3.32 \times 10^{-3}$

Answer 1

Answer: (C)

Given, $K_{C}=4 \times 10^{-6} mol / L$

$2 NOCl (g) \rightleftharpoons 2 NO (g)+ Cl _{2}(g)$

$\Delta n=$ product mole $-$ reactant mole

$=3-2=1$

From $K_{p}$ equation

$K_{p}=K_{C} \times(R T)^{\Delta n}$

$=4 \times 10^{-6} mol / L$

$\times\left(0.0831\, L \text { bar }\, k ^{-1}\, mol ^{-1}\right. \times 1000\, K )^{2}$

$K_{p}=3.32 \times 10^{-4}$ bar