Gibbs Free Energy
At 298 K, a reaction has ΔH = +25 kJ mol⁻¹ and ΔS = +120 J mol⁻¹ K⁻¹. Is the reaction spontaneous at 298 K?
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About This Question
- Subject
- chemistry
- Chapter
- chemical thermodynamics
- Topic
- gibbs free energy
- Difficulty
- Medium
- Year
- 2025
Solution
Correct Answer:
Yes, ΔG < 0
- Formula: ΔG=ΔH−TΔS.
- Values:
- ΔH=+25,000 J/mol.
- T=298 K.
- ΔS=+120 J/mol·K.
- Calculation:
- TΔS=298×120=35,760 J/mol.
- ΔG=25,000−35,760=−10,760 J/mol.
- Criterion for Spontaneity: If ΔG<0, the reaction is spontaneous.
- Conclusion: Since ΔG is negative, the reaction is spontaneous even though it is endothermic.
This medium difficulty chemistry question is from the chapter chemical thermodynamics, covering the topic of gibbs free energy. It appeared in the 2025 exam.
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