K_P for the following reaction is 3.0 at 1000 ~K . CO_2(~g)+C(s) leftharpoons 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 )

Correct answer: (B) 3.6 × 10^-2. CO_2(~g)+C(s) leftharpoons 2 CO(g) K_p=K_c ·(RT)^Δ n_g K_p=3.0 . R=0.083 ~L bar K^-1 ~mol^-1 Δ n_g =2-1=1 ∴ 3.0 =K_c(0.083 × 1000)^1 ~K_c=3/83=3.6 × 10^-2

Q62 / 200 · NEET 2022 (Phase 2) · Chemistry

$K_P$ for the following reaction is 3.0 at $1000 \mathrm{~K}$. $\mathrm{CO}_2(\mathrm{~g})+\mathrm{C}(\mathrm{s}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})$ What will be the value of $\mathrm{K}_C$ for the reaction at the same temperature? (Given: $\mathrm{R}=0.083 \mathrm{~L} \mathrm{bar} \mathrm{K}^{-1} \mathrm{~mol}^{-1}$ )

A
0.36
Correct answer
B
$3.6 \times 10^{-2}$
C
$3.6 \times 10^{-3}$
D
3.6

Solution

$\begin{aligned} & \text { } \mathrm{CO}_2(\mathrm{~g})+\mathrm{C}(\mathrm{s}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g}) \\ & \mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \cdot(\mathrm{RT})^{\Delta n_{\mathrm{g}}} \\ & \mathrm{K}_{\mathrm{p}}=3.0 . \mathrm{R}=0.083 \mathrm{~L} \mathrm{bar} \mathrm{K}^{-1} \mathrm{~mol}^{-1} \\ & \begin{aligned} \Delta n_g & =2-1=1 \\ \therefore \quad 3.0 & =\mathrm{K}_{\mathrm{c}}(0.083 \times 1000)^1 \\ & \mathrm{~K}_{\mathrm{c}}=\frac{3}{83}=3.6 \times 10^{-2} \end{aligned} \end{aligned}$

Hence, the correct answer is option: 'B'.

Solution

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