Multiple Choice
Determine if reaction is spontaneous under standard conditions, if not at what temperature will it be spontaneous?
3 A (g) + 5 B (s) → 3 AB (s) + B2 (g) ∆H° = 112.7 kJ, ∆S° = 78.3 J/K.
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19. Chemical Thermodynamics
Gibbs Free Energy Calculations
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Calculate ΔG° (in kJ) for a reaction where ΔH°= +63 kJ, ΔS°= +675 J/K, and T = 298 K. Use the formula ΔG° = ΔH° - TΔS°.
A
-138.15 kJ
B
+138.15 kJ
C
-63.00 kJ
D
+63.00 kJ
Verified step by step guidance1
Identify the given values: ΔH° = +63 kJ, ΔS° = +675 J/K, and T = 298 K.
Convert ΔS° from J/K to kJ/K by dividing by 1000, since 1 kJ = 1000 J. This gives ΔS° = 0.675 kJ/K.
Use the formula for Gibbs free energy change: ΔG° = ΔH° - TΔS°.
Substitute the values into the formula: ΔG° = 63 kJ - (298 K * 0.675 kJ/K).
Perform the multiplication and subtraction to find ΔG° in kJ.
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