An electrochemical cell has an Eocell of 1.50 V and transfers 1 mole of electrons. The Faraday constant is 96,485 C/mol e-. What is the value of delta G?

ΔG° = -1.45 × 10⁵ J

Explanation:

Step 1: Given data

Step 2: Calculate the standard Gibbs free energy change (ΔG°)

We will use the following expression.

ΔG° = -n × F × E°cell

ΔG° = -1 mol e⁻ × 96,485 C/mol e⁻ × 1.50 V

ΔG° = -1.45 × 10⁵ J

i'm pretty sure it is letter c.) car

the correct answer is:

a. formation of precipitation