Problem: Consider these hypothetical chemical reactions:A ⇌ B,     ΔG = 14.3 kJ/molB ⇌ C,     ΔG = –30.2 kJ/molC ⇌ D,     ΔG = 6.20 kJ/molWhat is the free energy, ΔG, for the overall reaction, A ⇌ D?

FREE Expert Solution

We can use Hess’s Law to determine the ΔG for the overall reaction, A ⇌ D


The given ΔG values are: 

A ⇌ B,     ΔG = 14.3 kJ/mol
B ⇌ C,     ΔG = –30.2 kJ/mol
C ⇌ D,     ΔG = 6.20 kJ/mol


Rearrange the reaction and adjust the ΔG° value accordingly:


Reaction 1: A is in the reactant in the final reaction. No change

A ⇌ B,     ΔG = 14.3 kJ/mol



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Problem Details

Consider these hypothetical chemical reactions:

A ⇌ B,     ΔG = 14.3 kJ/mol
B ⇌ C,     ΔG = –30.2 kJ/mol
C ⇌ D,     ΔG = 6.20 kJ/mol

What is the free energy, ΔG, for the overall reaction, A ⇌ D?

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