Question

Write chemical equations to represent the cathode, anode, and net cell reactions.

1) Cd | Cd(NO3)2 || Ag(NO3)2 | Ag

Reduction at Cathode: Cd2+ + 2e- ---> Cd
Oxidation at Anode: [Ag ---> Ag+ + e-] x2

Cd2+ + 2Ag ---> Cd + 2Ag2+

2) Pt | IO3-,H+ || Zn2+ | Zn

Reduction at Cathode: 2IO3- + 12H+ + 10e- ---> I2 + 6H2O
Oxidation at Anode: [Zn ---> Zn2+ + 2e-] x 5

2IO3- + 12H+ + Zn ---> I2 + 6H2O + Zn2+

Answer 1

For #1, have you done the voltage, Ecell?
Is this reaction to occur spontaneously?
If so, isn't what you show as the cell reaction a negative voltage? (The silver ion should be Ag^+.
The second equation isn't multiplied by 5 for Zn.

Answer 2

1) Cd | Cd(NO3)2 || Ag(NO3)2 | Ag

Reduction at Cathode: [Ag+ + e- ---> Ag]x2
Oxidation at Anode: Cd ---> Cd2+ + 2e-

2Ag+ + Cd ---> Ag + Cd2+

Is this right?
2IO3- + 12H+ + 5Zn ---> I2 + 6H2O + 5Zn2+

Answer 3

2Ag+ + Cd ---> 2Ag + Cd2+ *

Answer 4

For the cell reactions to occur spontaneously, you have equations written correctly and oxidized/reduced equations also are correct. You have omitted a 5 Zn on the left of the second cell and 5Zn^+2 on the right. But you showed it multiplied by 5; I assume the omission was just an oversight.