Hydrogen sulfide decomposes according to the following reaction
2H₂S(g) $\to$ 2H₂(g) + S₂(g)
For this reaction at 298K $\Delta$ S° = 78.1 J/K, $\Delta$ H° = 169.4 kJ,and $\Delta$ G° = 146.1 kJ.What is the value of $\Delta$ G° at 900 K?

Question

Hydrogen sulfide decomposes according to the following reaction
2H₂S(g)

\to

2H₂(g) + S₂(g)
For this reaction at 298K

\Delta

S° = 78.1 J/K,

\Delta

H° = 169.4 kJ,and

\Delta

G° = 146.1 kJ.What is the value of

\Delta

G° at 900 K?

Quizplus · Accepted Answer

The change in Gibbs free energy (ΔG°) with temperature can be estimated using the equation ΔG° = ΔH° - TΔS°. At 900 K, ΔG° = 169.4 kJ - 900 K * 0.0781 kJ/K = 99.1 kJ.

Hydrogen Sulfide Decomposes According to the Following Reaction 2H2S(g) →\to→ 2H2(g)+ S2(g) for This Reaction at 298K

Hydrogen Sulfide Decomposes According to the Following Reaction
2H₂S(g) $\to$ 2H₂(g)+ S₂(g)
for This Reaction at 298K