Tamil Nadu Board of Secondary EducationHSC Science Class 11th

# What is the equilibrium constant Keq for the following reaction at 400 K? 2NOClX(g)↽−−⇀2NOX(g)+ClX2X(g), given that H° = 77.2 kJ mol−1 and ∆S° = 122 JK−1 mol−1 - Chemistry

Numerical

What is the equilibrium constant Keq for the following reaction at 400 K?

$\ce{2NOCl_{(g)} ⇌ 2NO_{(g)} + Cl2_{(g)}}$, given that H0 = 77.2 kJ mol−1 and ∆S0 = 122 JK1 mol1

#### Solution

T = 400 K; ∆H0 = 77.2 kJ mol1 = 77200 J mol1;

∆S0 = 122 JK1 mol1
∆G0 = −2.303 RT log Keq

log Keq = (-∆"G"^0)/(2.303  "RT")

log Keq = ((-∆"H"^0 - "T"∆"S"^0))/(2.303  "RT")

log Keq = -((77200 - 400  xx 122)/(2.303 xx 8.314 xx 400))

log Keq = -((28400)/7659)

log Keq = − 3.7080

Keq = antilog (−3.7080)

Keq = 1.95 × 10−4

Concept: Gibbs Free Energy (G)
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#### APPEARS IN

Tamil Nadu Board Samacheer Kalvi Class 11th Chemistry Volume 1 and 2 Answers Guide
Chapter 7 Thermodynamics
Evaluation | Q II. 36. | Page 226
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