Solution Found!
Consider the rechargeable battery: Zn(s)
Chapter 13, Problem 13-10(choose chapter or problem)
Consider the rechargeable battery: Zn(s) | ZnCl2(aq) || Cl(aq) | Cl2(l) | C(s) (a) Write reduction half-reactions for each electrode. From which electrode will electrons flow from the battery into a circuit if the electrode potentials are not too different from E values? (b) If the battery delivers a constant current of 1.00 103 A for 1.00 h, how many kilograms of Cl2 will be consumed?
Questions & Answers
QUESTION:
Consider the rechargeable battery: Zn(s) | ZnCl2(aq) || Cl(aq) | Cl2(l) | C(s) (a) Write reduction half-reactions for each electrode. From which electrode will electrons flow from the battery into a circuit if the electrode potentials are not too different from E values? (b) If the battery delivers a constant current of 1.00 103 A for 1.00 h, how many kilograms of Cl2 will be consumed?
ANSWER:Step 1 of 3
(a)
Electrochemical cells are described by the notation in which single vertical line represents phase boundary and double vertical line represents the salt bridge.
The two electrodes are shown at the extreme left and right sides of the line diagram. Oxidation occurs at left side electrode (anode) and reduction occurs at right side electrode (cathode).
The line notation for the rechargeable battery as follows:
From the above line notation, zinc metal is oxidized at zinc electrode and chlorine is reduced at carbon electrode.
The reduction half reaction for each electrode are as follows:
