We’re being asked to calculate for ΔG° for the Ecell with the cell notation:

Cr|Cr ^{3+}||Hg _{2} ^{2+}|Hg(l)

**ΔG° can be calculated from the cell potential using the following equation:**

$\overline{){\mathbf{\u2206}}{\mathbf{G}}{\mathbf{=}}{\mathbf{-}}{\mathbf{nFE}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}}$

ΔG° = Gibbs Free Energy, J

n = # of e^{-} transferred

F = Faraday’s constant = 96485 J/(mol e^{-})

E°_{cell} = standard cell potential, V

**First, let’s determine ****the cell potential and the number of electrons transferred**** from the cell reaction:**

The value of E°cell for Cr|Cr ^{3+}||Hg _{2} ^{2+}|Hg(l) is 1.78 V. Calculate ΔG° for this reaction at 25 .

a. -1220 kJ

b. -1031 kJ

c. -872 kJ

d. -851 kJ

e. -621 kJ

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Cell Potential concept. If you need more Cell Potential practice, you can also practice Cell Potential practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty of*The value of E°cell for Cr|Cr 3+||Hg 2 2+|Hg(l) is 1.78 V. C...*as high difficulty.