Galvanic Cell Worksheet
Explore the principles of galvanic cells, including redox reactions, electrode potentials, and cell notation, with this comprehensive Grade 12 chemistry worksheet.
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Galvanic Cell Worksheet
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Read each question carefully and provide thorough answers. Show all your work for calculations.
1. In a galvanic cell, which electrode is where oxidation occurs?
Cathode
Anode
Salt bridge
External circuit
2. What is the purpose of the salt bridge in a galvanic cell?
To provide a path for electrons
To maintain electrical neutrality
To initiate the redox reaction
To prevent ion migration
1. A galvanic cell converts energy into energy.
2. The standard electrode potential for the reduction of Cu²⁺ to Cu is V.
1. Electrons flow from the cathode to the anode in a galvanic cell.
True
False
2. The cell potential (Ecell) of a galvanic cell must be positive for a spontaneous reaction.
True
False
1. Describe the function of a salt bridge in a galvanic cell and explain why it is necessary for continuous operation.
2. A galvanic cell is constructed using a zinc electrode in a 1.0 M Zn(NO₃)₂ solution and a nickel electrode in a 1.0 M Ni(NO₃)₂ solution. Given the standard reduction potentials: Zn²⁺(aq) + 2e⁻ → Zn(s) E° = -0.76 V and Ni²⁺(aq) + 2e⁻ → Ni(s) E° = -0.23 V. a) Write the balanced overall redox reaction for this cell. b) Calculate the standard cell potential (E°cell).
Match each term with its correct definition.
1. Anode
a. Site of reduction
2. Cathode
b. Negative electrode in a galvanic cell
3. Oxidation
c. Loss of electrons
4. Reduction
d. Gain of electrons