The δg°/' of the reaction is - "8.550" kj ·mol-1. calculate the equilibrium constant for the reaction. (assume a temperature of 25°

c.)

31.5. If ΔG° = - 8.550 kJ·mol^ (1) at 25 °C, K = 31.5.

The relationship between ΔG° and K is

ΔG° = - RTlnK

where

R = the gas constant = 8.314 J·K^ (-1) mol^ (-1)

T is the Kelvin temperature

Thus,

lnK = - ΔG° / (RT)

In this problem,

T = (25 + 273.15) K = 298.15 K#

∴ lnK = - [-8550 J·mol^ (-1) ]/[8.314 J·K^ (-1) mol^ (-1) x 298.15 K]

= [8550 J·mol^ (1) ]/[2479 J·mol^ (-1) ] = 3.449

K = e^3.449 = 31.5