For reactions carried out under standard-state conditions, the equation ΔG = ΔH - TΔS becomes ΔG° = H° - TΔS°. Assuming ΔH° and ΔS° are independent of temperature, one can derive the equation:
ln(K2/K1) = (ΔH°/R)((T2 - T1)/(T1T2))
where K1 and K2 are the equilibrium constants at T1 and T2, respectively. Given that at 25.0°C, Kc is 4.63 x 10^-3 for the reaction
N2O4(g) ⇌ 2NO2(g) ΔH° = 58.0 kJ/mol
calculate the equilibrium constant at 63.0°C.