Zinc reacts with dilute hydrochloric acid to give hydrogen at `17^(@)C`. The enthalpy of the reaction is `-12.00 kJ mol^(-1)` of zinc and entropy change equals `50 J K^(-1) mol^(-1)` for the reaction. Calculate the free enegry change and predict whether the reaction is spontaneous or not.

Explanation

Given, `DeltaH =- 12.00 kJ mol^(-1)`
`DeltaS = 5.0 J K^(-1) mol^(-1) = 0.005 k J^(-1) mol^(-1)`
`T = 17 +273 = 290 K`
Applying `DeltaG = DeltaH - T DeltaS`
`=- 12.00 - 0.005 xx 290`
`=- 12.00 - 1.45 =- 13.45 kJ mol^(-1)`
Since `DeltaG` is negative, the reaction will be spontaneous.