Hydrogen sulfide decomposes according to the following reaction
2H2S(g) → 2H2(g) + S2(g)
For this reaction at 298K:
ΔS° = 78.10 J/K,
ΔH° = 169.4 kJ,
and ΔG° = 146.1 kJ.
What is the value of ΔG° at 750 K?
*note: 1 kJ = 1000 J
Multiple Choice
• 48.4 kJ
• 110.8 kJ
• −69881 kJ
• 240 kJ
• 99.1 kJ