Question

The value of log₁₀K for a reaction $A \rightleftharpoons B$ is
(Given : $\Delta_rH^0_{ 298K}$ = -54.07 kJ mol⁻¹, $\Delta_rS^0_{ 298K}$ = 10 JK⁻¹ mol⁻¹ and R = 8.314 JK⁻¹ mol⁻¹; 2.303 × 8.314 × 298 = 5705)
(a) 5
(b) 10
(c) 95
(d) 100

Answer 1

(d) part is the correct option