Metal M forms soluble compound M(NO3)2. Solution is electrolyzed. When constant current 2.5amperes is applied?

for 35min, 3.06g of metal is deposited. Calculate the molar mass of M.
b) The metal identified in A is used with zinc to construct a galvanic cell. Write network ionic eq for the cell rxn & calculate the cell potential
c) Calculate delta G at 298K for rxn in module B
d) Calculate energy for chell from B if the initial concentration of ZnSO4 is .1M, but concentration of M(NO3)2 is same.

Please label these as to which division you are answering. thank you
Answers:
a) Calculate the molar mass of M.
35*60*2.5/(2*96485) = 0.02721 (mol)
M = 3.06g/0.02721mol = 112.5g/mol (element Cd)

b) The metal identified in A is used with zinc to construct a galvanic cell. Write web ionic eq for the cell rxn & calculate the cell potential
Cd(2+) + 2e- ==> Cd, E° =-0.76V
Zn(2+) + 2e- ==> Zn, E° = -0.40V
Zn + Cd(2+) ==> Zn(2+) + Cd, E° = -0.36V

c) Calculate delta G at 298K for rxn in member B
G = -nEF = 2*0.36*96485 = 69.5 (kJ)

d) Calculate energy for chell from B if the initial concentration of ZnSO4 is .1M, but concentration of M(NO3)2 is same.
E = E° -RT/nF Ln(Q)
= -0.36-(8.314*298/(2*96485))*Ln(0.1) = -0.330 (V)
G = -nEF = 2*0.330*96485 = 63.8(kJ)

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