Problem: Calculate the standard entropy, ΔS°rxn, of the following reaction at 25.0 °C using the data in this table. The standard enthalpy of the reaction, ΔH°rxn, is –44.2 kJ·mol–1.C2H4 (g) + H2O (l) → C2H5OH(l)Then, calculate the standard Gibbs free energy of the reaction, ΔG°rxn.

FREE Expert Solution

Step 1

S°rxn =S°product - S°reactantS°rxn =[1 mol C2H5OH160.7 J1 mol C2H5OH· K]                  - [1 mol C2H4219.3 J1 mol C2H4· K + 1 mol H2O70.0 J1 mol H2O· K]

ΔS°rxn = -128.6 J/K


View Complete Written Solution
Problem Details

Calculate the standard entropy, ΔS°rxn, of the following reaction at 25.0 °C using the data in this table. The standard enthalpy of the reaction, ΔH°rxn, is –44.2 kJ·mol–1.

C2H4 (g) + H2O (l) → C2H5OH(l)

Then, calculate the standard Gibbs free energy of the reaction, ΔG°rxn.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.