Answers to Problems - Chapter 13 (8th Ed.) or Chapter 14 (7th Ed.)
13-3
13-5
13-7
In a galvanic cell, the two half reactions are physically separated from one another.
Electrons are generated at the anode via an oxidation process. The electrons flow
through the circuit to the cathode, where reduction occurs.
In order for this to be a spontaneous process, a favourable change in the Gibbs energy
(i.e., < 0) must occur. Also, the salt bridge is key for making sure that there is not a
build up of charge in either half cell.
13-8
(a)
Fe(s) | FeO(s) | KOH (aq) | Ag2O | Ag(s)
FeO(s) + H2O + 2e- ⇌ Fe(s) + 2OHAg2O + H2O + 2e- ⇌ 2Ag(s) + 2OH(b)
Pb(s) | PbSO4(s) | K2SO4(aq) || H2SO4(aq) | PbSO4(s) | PbO2(s) | Pb(s)
PbSO4(s) + 2e- ⇌ Pb(s) + SO4 (2-)
PbO2 + 4H+ + SO4 (2-) + 2e- ⇌ PbSO4(s) + 2H2O
13-10 and 13-12
13-17
(a) Pt(s) | Br2(l) | HBr(aq, 0.10 M) || Al(NO3)3(aq, 0.010 M) | Al(s) 13-19
13-21
13-28
13-35
DO NOT DO: 13-42/14-42