19. Chemical Thermodynamics
Entropy Calculations
69PRACTICE PROBLEM
Assuming that all of the reactants and products and in their standard states, calculate the change in Gibbs free energy for each set of ΔH°rxn, ΔS°rxn, and T. Identify if each of the reactions is spontaneous or not at the given temperature.
i. ΔH°rxn = –87.0 kJ/mol; ΔS°rxn = –124 J/mol•K; and T = 925 K
ii. ΔH°rxn = –87.0 kJ/mol; ΔS°rxn = –124 J/mol•K; and T = 455 K
iii. ΔH°rxn = –87.0 kJ/mol; ΔS°rxn = –124 J/mol•K; and T = 298 K
iv. ΔH°rxn = +87.0 kJ/mol; ΔS°rxn = –124 J/mol•K; and T = 350 K
Assuming that all of the reactants and products and in their standard states, calculate the change in Gibbs free energy for each set of ΔH°rxn, ΔS°rxn, and T. Identify if each of the reactions is spontaneous or not at the given temperature.
i. ΔH°rxn = –87.0 kJ/mol; ΔS°rxn = –124 J/mol•K; and T = 925 K
ii. ΔH°rxn = –87.0 kJ/mol; ΔS°rxn = –124 J/mol•K; and T = 455 K
iii. ΔH°rxn = –87.0 kJ/mol; ΔS°rxn = –124 J/mol•K; and T = 298 K
iv. ΔH°rxn = +87.0 kJ/mol; ΔS°rxn = –124 J/mol•K; and T = 350 K