Recall: Cell Notation → "easy as ABC"
A = Anode
B = Barrier (||)
C = Cathode
Anode → Oxidation → Lose electrons
Cathode → Reduction → Gain electrons
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: please provide.
E°= 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 713 A for 30.0 min.
Answer must be in Kg.
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What scientific concept do you need to know in order to solve this problem?
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