K_P for the following reaction is 3.0 at 1000 K.
${CO}_{2} (g) + C (s) ⇌ 2 CO (g)$
What will be the value of K_C for the reaction at the same temperature?
(Given: R = 0.083 L bar K^-1 mol^-1)

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3.6

3.6 x 10^-3

3.6 x 10^-2

0.36

answer is C.

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Detailed Solution

$\begin{array}{l} {CO}_{2} (g) + C (s) ⇌ 2 CO (g) \\ Δn = 2 - 1 = 1 \\ K_{P} = K_{C} (RT)^{Δn} \\ K_{P} = K_{C} (RT)^{1} \\ [K_{P} = 3] \\ K_{C} = \frac{K_{P}}{RT} = \frac{3}{0.0821 \times 1000} = 0.036 \\ = 3.6 \times 10^{- 2} \end{array}$

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