Question

The standard free energy change in physiological conditions (G') for the reaction catalyzed by malate dehydrogenase in the citric acid cycle malate + NAD+ oxaloacetate + NADH + H+ is ~+29 kJmol-1 Calculate the actual G' at 37C if Keq' is 1.02 × 10-5

Answer 1

Answer: The actual value of
`\Delta G` is -618 J/mol

Step-by-step explanation:

Relation of ree energy change and equilibrium constant

`\Delta G=\Delta G^0+2.303* RT* \log K_(eq)`

where,

`\Delta G` = Free energy change

`\Delta G^o` = standard free energy change = +29 kJ/mol =

R = universal gas constant

T = temperature =
`37^0C=(37+273)K=310K`

`K_(eq)` = equilibrium constant =
`1.02* 10^(-5)`

`\Delta G=+29000J/mol+2.303* 8.314J/Kmol* 310K* \log (1.02* 10^(-5))`

`\Delta G=29000J/mol-29619J/mol=-618J/mol`

The actual value of
`\Delta G` is -618 J/mol