1) Calculate for the electrochemical cell below, Pb(s) |PbSO4(s) | Pb2+(aq) Ag+(
ID: 841652 • Letter: 1
Question
1)Calculate for the electrochemical cell below,
Pb(s) |PbSO4(s) | Pb2+(aq) Ag+(aq) | Ag(s)
given the following standard reduction potentials.
Ag+(aq) + e- ->Ag(s) E° = +0.799 V
PbSO4(s)+ 2e- -> Pb(s) + SO4 2-(aq) E = -0.356 V
a) -1.954 V
b) -1.155 V
c) +0.443V
d) +1.155 V
2) Consider the following half- reactions:
Cu2+ (aq) + 2e- --> Cu(s)E = +0.34 V
Sn2+(aq) + 2e- --> Sn(s) E = -0.14 V
Fe2+(aq) +2e- --> Fe(s)E = -0.44 V
Al3+(aq) +3e- --> Al(s) E = -1.66 V
Mg2+(aq) + 2e- --> Mg(s) E = -2.37 V
Which of the above metals or metal ions will reduce Fe2+ ?
a) Cu(s) and Sn(s)
b) Cu2+(aq) and Sn2+(aq)
c) Al3+(aq) and Mg2+ (aq)
d) Al(s) and Mg(s)
e) Sn(s) and Al3+ (aq)
3) The following reaction occurs spontaneously
2H+ (aq) +Ca(s) --> Ca2+(aq) + H2(g)
Write a balanced recuction half-reaction-
a) 2H+(aq) + 2e --> H2(g)
b) 2H+ (aq) --> H2(g) + 2e-
c) H2(g) --> 2H+(aq) + 2e-
d) Ca(s) + 2e- --> Ca2+(aq)
e) Ca(s) --> Ca2+(aq) + 2e-
Explanation / Answer
Pb(s) |PbSO4(s) | Pb2+(aq) Ag+(aq) | Ag(s)
given the following standard reduction potentials.
Ag+(aq) + e- ->Ag(s) E° = +0.799 V
PbSO4(s)+ 2e- -> Pb(s) + SO4 2-(aq) E = -0.356 V
answer ; a) -1.954 V
2) Consider the following half- reactions:
Cu2+ (aq) + 2e- --> Cu(s)E = +0.34 V
Sn2+(aq) + 2e- --> Sn(s) E = -0.14 V
Fe2+(aq) +2e- --> Fe(s)E = -0.44 V
Al3+(aq) +3e- --> Al(s) E = -1.66 V
Mg2+(aq) + 2e- --> Mg(s) E = -2.37 V
Which of the above metals or metal ions will reduce Fe2+ ?
answer : c) Al3+(aq) and Mg2+ (aq)
3) The following reaction occurs spontaneously
2H+ (aq) +Ca(s) --> Ca2+(aq) + H2(g)
Write a balanced recuction half-reaction-
answer : a) 2H+(aq) + 2e --> H2(g)
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