Gibbs Free Energy Equations

[Alexia Joseph 2B]

Can someone go over a summary of a situation you should use each Gibbs equation in?

[Joyce Lee 1C]

Gibbs Free Energy is defined as: G = H -TS
For a process at constant temperature:
ΔG = ΔH - T ΔS or (ΔG-T) = (ΔH/T) - ΔS
At constant temperature and pressure
ΔG = -T ΔStot
To find the Gibbs free energy of reaction, ΔG, using difference in molar Gibbs free energies, Gm
ΔG = ∑nGm (products) - ∑nGm (reactants)
To find standard Gibbs free energy, ΔG°, in terms of standard molar Gibbs energies
ΔG° = ∑nΔG°m (products) - ∑nΔG°m (reactants)
When a system is at equilibrium:
Gp° - Gr° = -RTln([P]/[R]) = -RTln(k)
When the system is not at equilibrium:
ΔG = Gp - Gr = Gp° - Gr° + RTln([P]/[R]) = ΔG° + RTln(Q)

I'm pretty sure there are more that I didn't include...

[Michelle Lee 2E]

In friday's lecture (and other prior unrelated lectures), Dr. Lavelle set two gibbs free energy equations equal to each other. Can we assume that we can set any of these equations for gibbs free energy equal to each other? (not standard gibbs free energy because that's not the same as just gibbs free energy)

[Mishta Stanislaus 1H]

In friday's lecture (and other prior unrelated lectures), Dr. Lavelle set two gibbs free energy equations equal to each other. Can we assume that we can set any of these equations for gibbs free energy equal to each other? (not standard gibbs free energy because that's not the same as just gibbs free energy)

I have the same question