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

To solve the problem, we will use the Gibbs free energy equation:

\[ \Delta G = \Delta H - T \Delta S \]

where:
- \(\Delta G\) = change in Gibbs free energy
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