Acritical 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)+ h20 (l) -> adp (aq) + hpo4 (negative two overall charge) (aq).

for which ? g�rxn = �30.5 kj/mol at 37.0 �c and ph 7.0. calculate the value of ? grxn in a biological cell in which [atp] = 5.0 mm, [adp] = 0.80 mm, and [hpo42�] = 5.0 mm.

a. what is the delta g rxn in kj/mol?

b. is the hydrolysis of atp spontaneous under these conditions?

A) The ΔG of the reaction is -48.9 kJ/mol.

B) yes, reaction will be spontaneous under these condition as ΔG is less than zero.

Explanation:

Given concentration of:

[ATP] = 5.0 mM = 0.005 M, [ADP] = 0.80 mM = 0.0008 M,

The reaction quotient is given by:

To calculate the ΔG(at 25°C) for given value of Gibbs free energy, we use the relation:

where,

= Gibbs free energy at given conditions

= Gibbs free energy at equilibrium=-30.5 kJ/mol

R = Gas constant =

T = temperature =

= reaction quotient at 37°C   = 0.0008

Putting values in above equation, we get:

The ΔG of the reaction is -48.9 kJ/mol. Yes, reaction will be spontaneous under these condition as ΔG is less than zero.

false

because it does not have the potential to be entirely used up

the answer is d. 74.02