Find out the value of K c for each of the following equilibria from the value of K p : (i) 2NOCl (g) ⇌ 2NO (g) + Cl 2 (g); K p = 1.8 × 10 –2 at 500 K (ii) CaCO 3 (s) ⇌ CaO(s) + CO 2 (g); K p = 167 at 1073 K

Question

Philoid · Accepted Answer

We know that,

K_p = K_c[RT]^Δn

Where Δn is number of gas molecule in products minus number of gas molecule in reactant in balanced chemical equation.

(i)

2NOCl (g) ⇌2NO (g) + Cl₂ (g)

Number of gaseous species on product side is 3 (2 NO and 1 Cl₂ ) and on reactant side is 2 (2 NOCl )

Thus, Δn = 3 - 2 = 1

T = 500 K

R = 0.0821 L atm K^-1

Given, K_p = 1.8 × 10^-2atm

∴ K_c =

=

= 4.4 × 10 �^-4mol L^-1

(ii)

CaCO₃ (s) ⇌CaO(s) + CO₂(g)

Number of gaseous species on product side is 1 (1 CO₂) and on reactant side is 0.

Thus, Δn = 1 – 0 = 1

T = 1073 K

K_p = 167 atm

K_c =

=

= 1.9 mol L^-1

Find out the value of Kc 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

Find out the value of K_c for each of the following equilibria from the value of K_p:
(i) 2NOCl (g) ⇌2NO (g) + Cl₂ (g); K_p= 1.8 × 10^–2 at 500 K

(ii) CaCO₃ (s) ⇌CaO(s) + CO₂(g); K_p= 167 at 1073 K