Problem: A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by ATP (aq) + H2O (l) → ADP (aq) + HPO 42- (aq)for which ΔG°rxn = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of ΔG  rxn (kJ/mol) in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.80 mM, and [HPO42-] = 5.0 mM. Is the hydrolysis of ATP spontaneous under these conditions?

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Problem Details

A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by

ATP (aq) + H2O (l) → ADP (aq) + HPO 42- (aq)

for which ΔG°rxn = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of ΔG  rxn (kJ/mol) in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.80 mM, and [HPO42-] = 5.0 mM.

Is the hydrolysis of ATP spontaneous under these conditions?

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Based on our data, we think this problem is relevant for Professor Cruickshank's class at NAU.