According to Gibbs Helmholtz equation
∆G = ∆H - T∆S, where
∆G = change in Gibbs energy
∆H = change in enthalpy, given as 400 kJ mol-1
∆S = change in entropy, given as 0.2 kJ K-1 mol-1
T = temperature at which reaction occurs
For a reaction to be spontaneous, ∆G < 0, means it must be negative.
If ∆G = 0, it is in equilibrium.
So, for reaction to be spontaneous, ∆G < 0; ∆H - T∆S < 0; ∆H < T∆S;
(∆H / ∆S) < T; 400 / 0.2 = 2000 K < T
This implies that the temperature must be more than 2000K for the reaction to be spontaneous.
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