Question

For a reaction $2 A(g) \rightleftharpoons 2 B(g)+C(g)$
$K_{C}=3.75 \times 10^{-6}$ at $1069 \,K .$ The approximate value of $K_{p}$ for this reaction at the same temperature is $\left(R=0.082 \,L\right.$ bar $mol ^{-1} \,K ^{-1}$ )

• A. $2.4 \times 10^{-4}$
• B. $3.3 \times 10^{-4}$
• C. $33 \times 10^{2}$
• D. $7.2 \times 10^{4}$

Answer 1

Answer: (B)

$K_{p}$ is related to $K_{C}$ by the formula.

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

For the equation $2 A ( g ) \rightleftharpoons 2 B(g)+C(g)$

$\Delta n=(2+1)-2=1$

$R =0.082 l \,\text { bar } mol ^{-1} K ^{-1}$

$T =1069 \,K $

$K_{C} =375 \times 10^{-6}$

Substituting the values in equation and solving we get $K_{p}=3.3 \times 10^{-4}$