The value of log_(10)K for a reaction A hArr B is ( Given :Delta _(r) H_(298K)^(@)= -54.07kJmol^(-1),Delta_(r)S_(298K)^(@) = 10J K^(-1)mol^(-1) andR = 8.314 JK^(-1) mol^(-1), 2.303 xx 8.314 xx 298 K = 5705)

The value of log_(10)K for a reaction A hArr B is ( Given :Delta _(r)

1.	The value of log_(10)K for a reaction A hArr B is ( Given :Delta _(r) H_(298K)^(@)= -54.07kJmol^(-1),Delta_(r)S_(298K)^(@) = 10J K^(-1)mol^(-1) andR = 8.314 JK^(-1) mol^(-1), 2.303 xx 8.314 xx 298 K = 5705)
Answer» 5 10 95 100 Solution :`DeltaG^(@) =DELTAH^(@) - T DELTA S^(@)= - 2.303 RT log _(10) K` `:.-2.303 RT log_(10) K= DeltaH ^(@)- T DeltaS^(@)` i.e., `-2.303 xx 8.314 xx 298 xx log_(10)K` `=- 54.07xx 1000- 298 xx 10` `-5705 log_(10)K =- 54070 - 2980 = - 57050` or `log_(10)K =10`