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Question
Zinc reacts with dilute hydrochloric acid to give hydrogen gas at 17 oC. The enthalpy change of the reaction is −12.55 kJ mol−1 and entropy change equals to 5.0 J K−1 mol−1 for the reaction. Calculate the free energy change and predict whether the reaction is spontaneous or not.
Zinc reacts with dilute hydrochloric acid to give hydrogen gas at 17 oC. The enthalpy change of the reaction is −12.55 kJ mol−1 and entropy change equals to 5.0 J K−1 mol−1 for the reaction. Calculate the free energy change and predict whether the reaction is spontaneous or not.
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Solution
The correct option is A −14.00 kJ mol−1, spontaneous
Given, △H=−12.55 kJmol−1
△S=5.0 JK−1mol−1
=0.005 kJK−1mol−1
T=17+273=290 K
And Gibbs free energy is given as
△G=△H−T △S
=−12.55−0.005×290
=−12.55−1.45
=−14.00 kJ mol−1
the free energy change is equals to −14.00 kJ mol−1
Since, △G is negative, the reaction will be spontaneous.
Given, △H=−12.55 kJmol−1
△S=5.0 JK−1mol−1
=0.005 kJK−1mol−1
T=17+273=290 K
And Gibbs free energy is given as
△G=△H−T △S
=−12.55−0.005×290
=−12.55−1.45
=−14.00 kJ mol−1
the free energy change is equals to −14.00 kJ mol−1
Since, △G is negative, the reaction will be spontaneous.
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