CHEM123 Lecture Notes - Royal Aircraft Factory F.E.2, Electrochemistry, Galvanic Cell

• School: University of Waterloo
• Department: Chemistry
• Course: CHEM123
• Professor: Christine Dupont

Document Summary

The equilibrium constants for the following reactions are given at 297 k. What is the correct shorthand notation for the cell depicted in the figure given below: pb(s) pb2+(aq) i (aq) pbi2(s) pb(s, pb(s) pb2+(aq) i (aq) pb(s, pb(s) pb2+(aq) i (aq) pbi2(s, pb(s) pb2+(aq) pb(s) pbi2(s) i (aq, none of these. +(aq) + fe2+(aq) n2(g) + fe (s) + 5 h+(aq: n2(g) + 4 ag(s) n2h5, fe2+(aq) + 2 ag(s) fe (s) + 2 ag+(aq) +(aq) + 4 ag+(aq: none of the reactions above is spontaneous. A galvanic cell is constructed from fe/fe2+ and pb/pb2+ half-cells (under standard conditions). Which electrode is the cathode: the fe electrode, the pb electrode, neither (you cannot construct a galvanic cell from these two half-cells) In which direction do positive ions in the salt bridge move: towards fe2+(aq, towards pb2+(aq) N2(g) + 5 h+(aq) + 4e n2h5.