Using the Gibb's energy change, $$\Delta $$G^o = +63.3 kJ, for the following reaction,

Ag₂CO_3(s) $$\rightleftharpoons$$ 2 Ag⁺_(aq) + CO₃^2$$-$$ _(aq)
the K_sp of Ag₂CO_3(s) in water at 25^oC is
(R = 8.314 J K^$$-$$1 mol^$$-$$1)

For a given exothermic reaction, K_p and K'_p are the equilibrium constants at temperatures T₁ and T₂, respectively. Assuming that heat of reaction is constant in temperature range between T₁ and T₂, it is readily observed that

For the reversible reaction,
N_2(g) + 3H_2(g) $$\rightleftharpoons$$ 2NH_3(g) + heat

The equilibrium shifts in forward direction

Given that the equilibrium constant for the reaction,
2SO_2(g) + O_2(g) $$\rightleftharpoons$$ 2SO_3(g)
has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature ?
SO_3(g) $$\rightleftharpoons$$ SO_2(g) + $${1 \over 2}$$ O_2(g)