Question

For the following battery: Cd(s) | CdCl2(aq) || Cl–(aq) | Cl2(l) | C(s) a) Write the...

For the following battery: Cd(s) | CdCl2(aq) || Cl–(aq) | Cl2(l) | C(s)

a) Write the reduction half reaction occuring at the C(s) electrode. Include physical states of reactants and products

C(s) electrode: _____________________ Eo = 1.4V

b) From which electrode will electrons flow from the battery into a circuit? Cd(s) electrode or C(s) electrode

c) Calculate the mass of Cl2 consumed if the battery delivers a constant current of 783A for 48.0 min (in kg)

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Answer #1

Cd(s) | CdCl2(aq) || Cl–(aq) | Cl2(l) | C(s)

a. reduction half reaction

Cl2 + 2e- ------> 2Cl-

b. Cd cell is oxidation half cell

Electrons are flow from Cd electrode to Cl2 half cell. Cd(s) electrode >>>>>>answer

c. Cl2 + 2e- ------> 2Cl-

W = MCt/ZF

Z = 2

M = 71g/mole

C = 783A

t   = 48min = 48*60 = 2880sec

W = MCt/ZF

W    = 71*783*2880/2*96500   = 829.6g    = 0.8296Kg >>>>answer

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