General Chemistry

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() + 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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