Here again is the balanced equation for the formation of hydrogen gas (H2(g)) that took place in the test tube when Zn(s) and HCl(aq) were combined: 2 HCl(aq) + Zn(s)--> H2(g) + ZnCl2(aq) This enthalpy and entropy values for this reaction are Δ H = − 80.7 k J and Δ S = 0.0140 k J K. If you perform this reaction at 25.0 degrees Celsius, what is the free energy change (in kJ) for this reaction? Round your answer to three significant figures
Here again is the balanced equation for the formation of hydrogen gas (H2(g)) that took place in the test tube when Zn(s) and HCl(aq) were combined:
2 HCl(aq) + Zn(s)--> H2(g) + ZnCl2(aq)
This enthalpy and entropy values for this reaction are Δ H = − 80.7 k J and Δ S = 0.0140 k J K. If you perform this reaction at 25.0 degrees Celsius, what is the free energy change (in kJ) for this reaction? Round your answer to three significant figures
Any reaction whether it will be spontaneous or not can be known from the change its Gibbs free energy . If it is negative then the reaction is spontaneous otherwise if it is positive then non spontaneous and if it is 0 then it is in equilibrium .
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