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.

The answers and solutions to practice problems are available to registered users only.

Click here to Register!

 

 

Check Also 

General Chemistry

Leave a Comment

1670600597