 Solution

ID: past-exam-of-the-chemistry-course-of-the-year-1-of-the-natural-sciences-course-of-the-university-of-cambridge/2021/paper-1/4/b/solution

E^{\circ} = E_{right}^{\circ} - E_{left}^{\circ} = 1.660 - (- 0.285) = 1.945 V .

With

n = 4

Δ_{r} G^{\circ} = - n F E^{\circ} = - 4 (96485) (1.945) = - 7.51 \times 1 0^{5} J mo l^{- 1} .

Thus the conventional forward reaction is spontaneous under standard conditions, dissolving CeO

_{2}

while oxidizing ethanol. Oxide deposition is its reverse and needs external electrical work; its intention does not change the sign convention.

 New to topics? Read the docs here!