The standard reaction enthalpy of the reaction: SnO 2 (s) + 2H 2 (g) ⇌ Sn(s) + 2H 2 O(g) is +120 kJ/mol and the standard reaction Gibbs function is +30 kJ mol -1 at 900 K. Assuming that both ΔH° and Δ

Question

The standard reaction enthalpy of the reaction: SnO₂(s) + 2H₂(g) ⇌ Sn(s) + 2H₂O(g) is +120 kJ/mol and the standard reaction Gibbs function is +30 kJ mol^-1 at 900 K. Assuming that both ΔH° and ΔS° remain constant, estimate the minimum temperature (in Kelvin) above which the equilibrium constant becomes greater than one.

Answer:

1200.00

Solution:

ΔG° = ΔH° - TΔS° 30 = 120 - (900)ΔS°, so ΔS° = 90/900 = 0.1 kJ/mol/K

K > 1 requires ΔG° < 0, so T > ΔH°/ΔS°

T > 120/0.1 = 1200 K

Answer is 1200

TestHub · Accepted Answer

ΔG° = ΔH° - TΔS° 30 = 120 - (900)ΔS°, so ΔS° = 90/900 = 0.1 kJ/mol/K K > 1 requires ΔG° < 0, so T > ΔH°/ΔS° T > 120/0.1 = 1200 K Answer is 1200

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