Difference between ΔG = 0 and ΔG° = 0?

Moderators: Chem_Mod, Chem_Admin

Hannah Lee 2F
Posts: 117
Joined: Thu Jul 11, 2019 12:15 am

Difference between ΔG = 0 and ΔG° = 0?

Postby Hannah Lee 2F » Fri Feb 28, 2020 6:26 pm

At ΔG = 0, the reaction is in equilibrium. What is the difference between ΔG = 0 and ΔG° = 0?

Pegah Nasseri 1K
Posts: 100
Joined: Wed Feb 27, 2019 12:15 am

Re: Difference between ΔG = 0 and ΔG° = 0?

Postby Pegah Nasseri 1K » Fri Feb 28, 2020 7:05 pm

ΔG° is the change in gibbs free energy of formation, which is calculated using the equation ΔG°= -RTlnK. This is the gibbs free energy that occurs at equilibrium. ΔG takes into account ΔG°in its calculation: ΔG = ΔG°+ RTlnQ. Looking at the equation, just because ΔG°= 0, this doesn't necessarily mean that ΔG=0. The same is true for if ΔG=0, ΔG° doesn't necessary have to be 0. ΔG=0 just indicates that the reaction is at equilibrium while ΔG°= 0 shows that the equilibrium constant, K, is equal to 1 using the equation ΔG°= -RTnK = -RTln(1) = 0.

Return to “Gibbs Free Energy Concepts and Calculations”

Who is online

Users browsing this forum: No registered users and 0 guests