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) + H_2O(l) rightarrow ADP(aq) + HPO_4^2-(aq) for which Delta G degree _rxn = -30.5 kJ/mol at 37.0 degree C and pH 7.0. Calculate the value of Delta G_rxn in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.20 mM, and [HPO_4^2-] = 5.0 mM. Delta G_rxn Is the hydrolysis of ATP spontaneous under these conditions?

Explanation / Answer

convert everything into the units you will need.
temp 37.0*27=310K
5.0mM is millimolar and you need molar so
5.0/1000= 0.0050
0.2M/1000= 0.0001M
R= 8.314J/mo*k 0.008314kj/mol*k

now plug everything in to the equation
dG= -30.5+ (0.008314*310*In 0.00500.0002/0.0050)
dG= -30.5 + (0.008314*310*In 0.00020 )
dG= -30.5 + (-16.01)
dG= -46.51

2) Yes because dG is negative

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