Answer:
K = 2.21 × 10⁻³
Explanation:
The Gibbs free energy change (ΔG°) at a temperature T = 2400 K is 1.22 × 10⁵ J/mol. We can calculate the equilibrium constant (K) using the following expression.
[tex]\Delta G\°=-R.T.lnK[/tex]
where,
R is the ideal gas constant (8.314 J/mol.K)
T is the absolute temperature
[tex]\Delta G\°=-R.T.lnK\\lnK=\frac{-\Delta G\°}{R.T} =\frac{-1.22 \times 10^{5}J/mol}{(8.314J/K.mol).2400K} \\K=2.21 \times 10^{-3}[/tex]
