Question

the value of ΔG° for the phosphorylation of glucose in glycolysis is 13.8kJ/mol. find the value of Kc at 298K?

Answer 1

Answer : The value of $K_c$ at 298 is, $3.81\times 10^{-3}$

Solution :

Formula used :

$\Delta G^o=-2.303\times RT\times \log K_c$

where,

$\Delta G^o$ = Gibbs free energy = 13.8 kJ/mole

R = universal gas constant = 8.314 J/K/mole

T = temperature = 298 K

$K_c$ = equilibrium constant = ?

Now put all the given values in this formula, we get the value of $K_c$

$13.8\times 10^3J/mole=-2.303\times (8.314 J/K/mole)\times (298K)\times \log K_c$

$K_c=3.81\times 10^{-3}$

Therefore, the value of $K_c$ at 298 is, $3.81\times 10^{-3}$