For some reaction carried out at constant atmospheric pressure and at a constant temperature of 25◦C, it is found that ∆H = - 38.468 kJ/mol and ∆S = + 51.4 J mol · K. What is the value of ∆G for this reaction under these conditions?

Question

Chemistry

Jay Walton

16 October, 08:38

For some reaction carried out at constant atmospheric pressure and at a constant temperature of 25◦C, it is found that ∆H = - 38.468 kJ/mol and ∆S = + 51.4 J mol · K. What is the value of ∆G for this reaction under these conditions?

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Answers (1)

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Macey Middleton · Answer 1

Answer: ΔG = 23.169kJ/mol

Explanation:

Solution

To Calculate Gibbs free energy ΔG for the reaction above we use the equation ΔG=ΔH-TΔS.

Where

ΔH = 38.468 kJ/mol = 38468 J/mol

∆S = + 51.4 J mol-1 K-1).

T = 25◦C = 298k

ΔG = 38468J/mol-298k (51.4 J mol-1 K-1).

ΔG = 38468 J/mol - 15317.2J/mol

ΔG = 23168.8J/mol

ΔG = 23.169kJ/mol