Answer:
Here's what I get Ā
Explanation:
(i) Voltaic cell
A voltaic cell is a device that uses a chemical reaction to produce electrical energy.
(ii) Overall Cell Potential
The standard reduction potentials for the half-reactions are
Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā ā°Ā°/V
CuĀ²āŗ + 2eā» ā Cu Ā Ā 0.34
ZnĀ²āŗ + 2eā» ā Zn Ā -0.76
The half-reaction with the more positive potential is the reduction half-reaction. It is the reaction that occurs at the cathode.
The half-reaction with the more negative potential is the oxidation half-reaction. It is the Ā reaction that occurs at the anode.
We reverse that half-reaction and subtract the voltages to get the cell reaction.
Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā Ā ā°Ā°/V
Cathode: Ā CuĀ²āŗ + 2eā» ā Cu Ā Ā Ā Ā Ā Ā Ā 0.34
Anode: Ā Ā Zn ā ZnĀ²āŗ + 2eā» Ā Ā Ā Ā Ā Ā Ā -0.76
Cell: Ā Ā Ā Ā Ā Zn + Ā CuĀ²āŗ ā ZnĀ²āŗ + Cu Ā Ā 1.10
[tex]\mathcal{E}_{\text{cell}}^{\circ} = \mathcal{E}_{\text{cat}}^{\circ} - \mathcal{E}_{\text{an}}^{\circ} = \text{0.34 V} - \text{(-0.76 V)} = \text{0.34 V} + \text{0.76 V} = \textbf{1.10 V}[/tex]
(iii) Diagram
The specific labels will depend on your textbook.
They are often as follows.
a. Electron flow
b. Voltmeter or lightbulb
c. Electron flow
d. Cathode or Cu
e. CuĀ²āŗ(aq) and NOāā»(aq)
f. Salt bridge
g. ZnĀ²āŗ(aq) and NOāā»(aq)
h. Anode or Zn
The salt bridge enables ions to flow in the internal circuit and to maintain electrical neutrality in the two compartments.
It often consists of a saturated solution of KCl.
As ZnĀ²āŗ ions form in the anode compartment, Clā» ions move in to provide partners for them.
As CuĀ²āŗ ions are removed from the cathode compartment, Kāŗ ions move in to replace them.
Ā
Answer:a. Electron flow
b. Voltmeter or lightbulb
c. Electron flow
d. Cathode or Cu
e. CuĀ²āŗ(aq) and NOāā»(aq)
f. Salt bridge
g. ZnĀ²āŗ(aq) and NOāā»(aq)
h. Anode or Zn
Explanation:
