For a reactio, `Delta H= - 10000 " J. mol"^(-1) and Delta S = - 33.3 " J. mol"^(-1). K^(-1)`.
At what temperature will the reaction procees spontaneously from (i) left to right : (ii) right to left ?

Explanation

Equilibrium temperature, `T= (|Delta|)/(|Delta S|)= (10^(4))/(33.3)= 300.3 K `
(i) At 300.3 K, `T Delta S= 300.3xx(-33.3)= - 9.99 kJ` So, below 300.3 K, `|Delta H| gt |T Delta S|`, and hence `Delta G gt 0`. Therefore, the reaction will occur spontaneously from left to right below 300.3 K
(ii) Above `300.3 K, |Delta H| lt | T Delta S|` & hence `Delta G lt 0` . So, the reaction will occur spontaneously from right to left above 300.3 K.