Question

Following reaction is carried out at 398 K, 

2NO(g) + O₂(g)  2NO₂(g) 

At 298 K, Gibb's free energy of formations of NO (g) is 86.6 kJ/mol. What will be standard Gibb's free energy of NO₂(g) at 298 K? (Kp = 1.6 × 1012) 

(a) R (298) ln (1.6 × 1012) - 86600 

(b) 86600 + R (298) In (1.6 × 1012) 

(c) 86600 \(-\frac{In(1.6\times 10^{12})}{R(298)}\)

(d) 0.5 [2 × 8,6600 - R (298) In (1.6 × 1012)]

Answer 1

Correct option is : (d) 0.5 [2 × 8,6600 - R (298) In (1.6 × 1012)]