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Suppose the reaction A + B --> C + D has a Δ G of +...

Suppose the reaction A + B --> C + D has a Δ G of + 5.2 kcal/mol. If this reaction is coupled to the reaction ATP + H2O --> ADP + Pi, which has a Δ G of -7.3 kcal/mol. What will be the change in free energy of the combined reaction, and will the reaction be spontaneous? Explain your answer.

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Answer #1

A    +    B ------------------------> C   +    D ΔG =   + 5.2 kcal/mol.

ATP   +   H2O -----------------------> ADP + Pi ΔG =   -7.3 kcal/mol

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A + B + ATP + H2O --------------> C + D+ ADP + Pi       ΔG =   - 2.1 kcal/mol

ΔG =   -2.1 kcal/mol . is negative. so reaction is spontenous.

if delta G is positive then the reaction is non-spontaneous.

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