Question

Given the electrochemical cell reaction: ( Δ G = -nFE ), solve for E.

A. E = Δ G/nF
B. E = nF/Δ G
C. E = - ΔG/nF
D. E = -nF/Δ G

Answer 1

For the electrochemical cell reaction equation ΔG = -nFE, E is solved by rearranging the equation to E = -ΔG/nF, indicating answer C is correct.

Step-by-step explanation:

To solve for E in the electrochemical cell reaction formula ΔG = -nFE, we can rearrange the equation as follows:

• First, divide both sides of the equation by -nF to isolate E on one side.
• This gives us E = ΔG / -nF.

Thus the correct answer is C: E = -ΔG/nF.

In context, n represents the number of moles of electrons transferred, F is Faraday's constant, and ΔG is the change in free energy. A negative ΔG indicates a spontaneous reaction, and the value of cell potential E tells us about the voltage produced by the cell.