17. For the reaction at 298 K, 2A + B → C
ΔH = 400 kJ mol–1 and ΔS = 0.2 kJ K–1 mol–1
At what temperature will the reaction become spontaneous considering ΔH and ΔS to be constant over the temperature range?
17. For the reaction at 298 K, 2A + B → C
ΔH = 400 kJ mol–1 and ΔS = 0.2 kJ K–1 mol–1
At what temperature will the reaction become spontaneous considering ΔH and ΔS to be constant over the temperature range?
17. As per the Gibbs Helmholtz's equation:
ΔG = Δ H - TΔ S
For ΔG=0;
ΔH=TΔS
Or T=ΔH/ΔS
T = (400 KJ mol-1)/ (0.2 KJ K-1 mol-1)
= 2000 k
Thus, reaction will be in a state of equilibrium at 2000 K and will be spontaneous above this temperature
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