Question

What is produced at each electrode in the electrolysis of AgF(aq)? Match the products with the correct bin

products=H2(gas), O2(g), F2(g), Ag(s)

Bins-anode bin, cathode bin, not produced bin.

Given Reduction half-reaction Potential (V)

F2(g)+2e−→2F−(aq) +2.87

O2(g)+4H+(aq)+4e−→2H2O(l) +1.23

Br2(l)+2e−→2Br−(aq) +1.07

Ag++e−→Ag(s) +0.80

2H2O(l)+2e−→H2(g)+2OH−(aq)−0.83

Na+(aq)+e−→Na(s) −2.71

Answer 1

AgF consists of Ag+ and F- ions, which are fully dissociated in aqueous solution. When solving electrolysis problems, it is important to remember that water itself may also be subject to electrolysis. Thus, determining which species is oxidized and which species is reduced depends on selecting the processes that are the most energetically favorable. In this case we have two possible reductions and two possible oxidations, listed here along with their reduction or oxidation potentials:

Reduction:
2H+ + 2e- ==> H2, E = 0.00 V

Ag+ + e- ==> Ag, E = 0.8 V

Oxidation:
2F- ==> F2 + 2e-, E = -2.87 V

2H2O ==> O2 + 4H+ + 4e-, E = -1.23 V

The reactions with the *most positive* potentials are most likely to proceed. Therefore, the reduction of Ag+, which occurs at the cathode, is the most favorable reduction reaction and the oxidation of H2O, which occurs at the anode, is the most favorable oxidation reaction. Consequently, the major products of this hydrolysis are Ag and O2, whereas H2 and F2 are not produced in appreciable amounts.

cathode - Ag (s)

anode - O2 (g)