↓ E° → oxidation → anode
↑ E° → reduction → cathode
Oxidation: Cd(s) ⇌ Cd2+ (aq) + 2 e-
Reduction: Cl2 (l) + 2 e-⇌ 2 Cl-(aq)
b. Anode → electrons are generated via oxidation → electrons will flow from anode to cathode
Anode is Cd(s)
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 stales of reactants and products)
C(s) electrode_________________ E degree =1.4 V
(b) From which electrode will electrons flow from the battery into a circuit?
a) Cd(s) electrode
b) C(s) electrode
(c) Calculate the mass of Cl2 consumed if the battery delivers a constant current of 617 A for 83.0 min.
Complete this table relating the values of E°cell and ΔG° to K.
>0 , =0, <0
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