The equilibrium constant for a reaction is 10. What will be the value of ? R = 8.314 JK^–1 mol^–1, T = 300 K.

Using,

∆G = -RTlnK

⇒ ∆G = -2.303RTlogK

∆G = change in Gibbs energy

R = 8.314 × 10^-3 kJ mol^-1 K^-1 - constant

T = temperature; given as 300K

K = equilibrium constant

Substituting the above values

∆G = -2.303 × 8.314 × 10^-3 × 300 × log 10

∆G = -5.744 kJ mol^-1