19. Chemical Thermodynamics
Gibbs Free Energy
19. Chemical Thermodynamics Gibbs Free Energy
136PRACTICE PROBLEM
The reaction below represents the decomposition of a generic diatomic molecule in its standard state.
1/2 A2(g) → A(g)
Assuming that the standard molar Gibbs energy of formation of A(g) is 8.12 kJ•mol–1 at 2500 K and –72.20 kJ•mol–1 at 3500 K. Calculate the value of K (thermodynamic equilibrium constant) at each temperature.
Determine the value of ΔH°rxn for these data assuming that ΔH°rxn is independent of temperature.
The reaction below represents the decomposition of a generic diatomic molecule in its standard state.
1/2 A2(g) → A(g)
Assuming that the standard molar Gibbs energy of formation of A(g) is 8.12 kJ•mol–1 at 2500 K and –72.20 kJ•mol–1 at 3500 K. Calculate the value of K (thermodynamic equilibrium constant) at each temperature.
Determine the value of ΔH°rxn for these data assuming that ΔH°rxn is independent of temperature.