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Question
The Gibbs free energy change for the reaction for which ΔH=−393.4kJ and ΔS=−2.9JK−1mol−1 at 298K is:
The Gibbs free energy change for the reaction for which ΔH=−393.4kJ and ΔS=−2.9JK−1mol−1 at 298K is:
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Solution
The correct option is A −392.5kJ
ΔG=ΔH−TΔS
Given, ΔH=−393.4 kJ/mol and ΔS=−2.9 JK−1mol−1
ΔG=−393400−298×2.9=−392535.8 J≈−392 kJ
Hence, option B is correct.
ΔG=ΔH−TΔS
Given, ΔH=−393.4 kJ/mol and ΔS=−2.9 JK−1mol−1
ΔG=−393400−298×2.9=−392535.8 J≈−392 kJ
Hence, option B is correct.
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