The standard biological reaction Gibbs energy for the removal of the phosphate group from adenosine monophosphate is 14 kJ mol-1 at 298 K. What is the value of the thermodynamic standard reaction Gibbs energy?

The thermodynamic standard reaction Gibbs energy has been 284 kJ/mol.

The standard Gibbs free energy has been the energy required for changing the state of 1 mole of substance from its standard state.

The Gibbs free energy () has been given by:

Where,

R = constant = 0.008314 kJ.mol/K

T = temperature = 298 K

In K = natural log of K

Substituting the values for the calculation of K:

Taking the anti log on both the side:

K = 284 kJ/mol

The thermodynamic standard reaction Gibbs energy has been 284 kJ/mol.

For more information about the Gibbs energy, refer to the link:

link

K = 284

Explanation:

Gibbs free energy (DG) = RT(InK)

Where :

R = Gas constant = 8.314J/K/mol = 0.008314KJmol/K

T = temperature in Kelvin = 298K

K = dissociation rate

DG = 14

DG = RT(InK)

14 = 0.008314 × 298 × (InK)

14 = 2.477572 × InK

Ink = (14 ÷ 2.477542)

InK = 5.6507619

K = 284

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