Would my answers be correct?

Question

Build a voltaic cell with one beaker containing a solution of nickel (II) nitrate - Ni(NO3)2 - with a nickel electrode, and a second beaker containing a solution of zinc chloride - ZnCl2 - with a zinc electrode.

 a. The half reactions 

 b. Flow of electrons 

 c. Short-form notation 

 d. Electric potential (voltage)

a.

Zn + 2Cl- = ZnCl2 + 2e-

Ni(NO3)2 + 2e- = Ni2+ 2Ni(NO3)

b.

Ni2+ + 2e- → Ni(s)

Zn(s) → Zn2+ + 2e-

c.

Ni(s) | Ni(NO3)2(aq) || ZnCl2(aq) | Zn(s)

d.

E° cell = E° cathode - E° anode

E° cathode : Ni2+(aq) + 2e-1 → Ni(s) - 0.25 

E° anode: Zn2+(aq) + 2e-1 → Zn(s) - 0.76

E° cell = (-0.25) - (-0.76) 

= 0.51 V

Answer 1

Looks good but I'd maybe answer part (a) a little differently. Here's the way I'd do it.

a) Ni²⁺ + 2e- ==> Ni oxidation half reaction (anode)

Zn ===> Zn²⁺ + 2e- reduction half reaction (cathode)

b) for the flow of electrons, I think maybe they are asking to show the electrons from from the anode to the cathode.

c) and d) look fine to me.