Calculate kp at 298.15 k for the reactions (a), (b), and (c) using δg°f values.

(a) 2NO (g) + O₂ (g) ⇄2NO₂ (g) kp

(b) 2N₂O (g) ⇄2NO (g) + N₂ (g) kp

(c) N₂ (g) + O₂ (g) ⇄ 2NO (g) kp

Now A is

2NO + O₂⇄2NO₂

ΔG° = ΔG° products - ΔG reactants

=2 * 51.3 - (256.6)

-70.6kJ/mol.

ΔG° = - RT Inkp

-70.6 = - 8.314 * 10⁻³ ˣ 298.15 ˣInkJ

InkJ = 28.48

kp=2.34 ˣ 10¹²

B is

ΔG° = 2 * 86.6 - 2 * 104.2 = - 35.2

-35.2 = 8.314 * 10⁻³ ˣ 298.15 ˣInkJ

InkJ = 14.2

kp = 1.47ˣ 10⁶

C is

It is also similar

kp = 4.62 ˣ 10⁻³I