Standard Cell Potential & the Equilibrium Constant: Videos & Practice Problems

What is the relationship between galvanic cells and equilibrium?

How does the Nernst equation help in calculating cell potential under non-standard conditions?

Given a standard cell potential of 0.76 V and n = 2, calculate the equilibrium constant K.

Analyze how Gibbs free energy (ΔG) is related to the equilibrium constant (K) and standard cell potential (E°_cell).

Calculate ΔG at 298 K for a reaction with an equilibrium constant K = 100.

Calculate ΔG for a reaction with n = 3, F = 96485 C/mol, and E°_cell = 1.5 V.

How do you calculate the standard cell potential using the potentials of the cathode and anode?

Evaluate the use of the Nernst equation when the concentration of reactants is 0.5 M.

What happens to the reaction quotient (Q) as a chemical reaction reaches equilibrium?

Synthesize the relationship between cell potential, equilibrium constant, and Gibbs free energy in a reaction with E°_cell = 0.5 V, n = 2, and K = 10⁵.

What happens to the cell potential of a galvanic cell at equilibrium?

What role does the number of electrons transferred (n) play in the Nernst equation?

If the standard cell potential is 1.1 V and n = 4, what is the equilibrium constant K?

How does the equilibrium constant (K) affect Gibbs free energy (ΔG) in a chemical reaction?

Calculate ΔG at 298 K for a reaction with an equilibrium constant K = 0.01.

What is the standard cell potential if the cathode potential is 0.34 V and the anode potential is -0.76 V?

Evaluate the use of the Nernst equation when the concentration of products is 2 M.

What is the significance of the transition from Q to K in a chemical reaction?

Synthesize the relationship between cell potential, equilibrium constant, and Gibbs free energy in a reaction with E°_cell = 0.9 V, n = 3, and K = 10³.