Find out the value of K c for each of the following equilibria from the value of Kₚ: (i) 2NOCl(g) ⇌ 2NO(g) + Cl₂(g); Kₚ = 1.8 × 10⁻² at 500 K (ii) CaCO₃(s) ⇌ CaO(s) + CO₂(g); Kₚ = 167 at 1073 K

(i) K c = 4.33 × 10⁻⁴ (ii) K c = 1.87 — To find K c from Kₚ, we use the relation Kₚ = K c (RT)^(Δ n), which gives K c = Kₚ(RT)^(Δ n). Here, R = 0.0831 L bar K⁻¹ mol⁻¹. For the first reaction, Δ n = 1. For the second reaction, which is a heterogeneous equilibrium, pure solids are not included in the equilibrium expression, so Δ n = 1 as well.

Find out the value of K c for each of the following equilibria from…

Question 5 of 69intermediate🔧 ApplyNumerical2 marks

Find out the value of $K_c$ for each of the following equilibria from the value of $K_p$ : (i) $2NOCl(g) \rightleftharpoons 2NO(g) + Cl_2(g)$ ; $K_p = 1.8 \times 10^{-2}$ at 500 K (ii) $CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)$ ; $K_p = 167$ at 1073 K

(i)

Answer

$K_c = 4.33 \times 10^{-4}$

(ii)

Answer

$K_c = 1.87$

Explanation

To find $K_c$ from $K_p$ , we use the relation $K_p = K_c(RT)^{\Delta n}$ , which gives $K_c = \frac{K_p}{(RT)^{\Delta n}}$ . Here, $R = 0.0831$ L bar K $^{-1}$ mol $^{-1}$ . For the first reaction, $\Delta n = 1$ . For the second reaction, which is a heterogeneous equilibrium, pure solids are not included in the equilibrium expression, so $\Delta n = 1$ as well.

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