A critical reaction in the production of energy to do work or drive chemical rea

Question

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(t) ADP(aq) + HPO (aq) for which delta G degree rxn = -30.5kj/mol at 37.0 degree C are ph 7.0. Calculate the value of delta G rxn in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.90 mM, and [HPO ] = 5.0 mM delta G rxn = is the hydrolysis of ATP spontaneous under these conditions?

Explanation / Answer

We know that,

delta G = delta G0 + RT ln Q

where,

delta G = free energy at any moment

delta G0 = standard-state free energy

R is the ideal gas constant = 8.314 J/mol-K

T is the absolute temperature (Kelvin)

ln Q is natural logarithm of the reaction quotient

Q = [ADP] [HPO4 2-] / [ATP]

=> Q = 0.9 x 10^-3 x 5 x 10^-3 / 5 x 10^-3 = 9 x 10^-4

=> ln Q = -7.013

Therefore,

delta G = -30500 + 8.314 x 310 x (-7.013)

=> delta G = - 48575.2 J/mol = - 48.575 KJ/mol

Since delta G < 0, the reaction will be Spontaneous

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