Calculate the cell potential for each redox reaction and determine if it is spontanesous or not:
a) Zn(s) + Pb2+(aq) → Zn2+(aq) + Pb(s)
b) 2Cl–(aq) + Pb2+ (aq) → Cl2(l) + Pb(s)
c) Cd(s) + Pb2+(aq) → Cd2+(aq) + Pb(s)
d) Fe(s) + 3Ag+(aq) → Fe3+(aq) + 3Ag(s)
e) Ca2+(aq) + Fe(s) → Ca(s) + Fe2+(aq)
f) Ni(s) + Mg2+(aq) → Ni2+(aq) + Mg(s)
g) Sn2+(aq) + Mg(s) → Sn(s) + Mg2+(aq)
h) Br2(l) + 2I–(aq) → 2Br–(aq) + I2(s)
i) 2Al(s) + 3Cu2+(aq) → 2Al3+(aq) + 3Cu(s)
j) O2(g) + 4H+(aq) + Cu(s) → Cu2+(aq) + 2H2O(l)
k) MnO2(s) + 4H+(aq) + Cd(s) → Mn2+(aq) + 2H2O(l ) + Cd2+(aq)
To calculate the cell potential, we need to separate the reaction into half-reactions and look up the value for each cell potential in the table of standard reduction potentials.
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