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Questions and Answers
What is the primary function of the salt bridge in a voltaic cell?
What is the primary function of the salt bridge in a voltaic cell?
Which statement accurately describes the process of oxidation in a voltaic cell?
Which statement accurately describes the process of oxidation in a voltaic cell?
Which of the following components directly connects the two half-cells in a voltaic cell?
Which of the following components directly connects the two half-cells in a voltaic cell?
What happens to zinc metal in the voltaic cell as the reaction proceeds?
What happens to zinc metal in the voltaic cell as the reaction proceeds?
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In the cell notation Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s), what does '||' signify?
In the cell notation Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s), what does '||' signify?
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Which species acts as the reducing agent in the voltaic cell described?
Which species acts as the reducing agent in the voltaic cell described?
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What is the result of the overall redox reaction in the voltaic cell?
What is the result of the overall redox reaction in the voltaic cell?
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Which of the following correctly defines reduction in the context of the voltaic cell?
Which of the following correctly defines reduction in the context of the voltaic cell?
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Study Notes
Voltaic Cells
- Voltaic cells use a chemical reaction to produce electricity.
- Voltaic cells utilize oxidation-reduction reactions.
- A battery is a common example of a voltaic cell.
Basic Voltaic Cell Setup
- Two beakers, each containing a solution: one with zinc sulfate and the other with copper sulfate.
- A piece of zinc metal is placed in the zinc sulfate solution.
- A piece of copper metal is placed in the copper sulfate solution.
- A wire connects the zinc and copper metal, causing electrons to flow from zinc to copper.
- A salt bridge connects the two solutions.
Electron Movement
- Copper ions (Cu2+) have a stronger pull for electrons than zinc atoms.
- Zinc atoms lose electrons, becoming zinc ions (Zn2+) that dissolve in the solution.
- The lost electrons travel through the wire to the copper.
- Copper ions in the solution gain electrons, becoming neutral copper atoms that attach to the copper metal.
- This electron movement creates an electric current.
Oxidation and Reduction
- Oxidation: Loss of electrons, occurs at the anode (zinc metal).
- Reduction: Gain of electrons, occurs at the cathode (copper metal).
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Half Reactions:
- Oxidation: Zn(s) → Zn2+(aq) + 2e-
- Reduction: Cu2+(aq) + 2e- → Cu(s)
- Net Ionic Equation: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
Cell Notation
- A shorthand representation of the voltaic cell:
- Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s)
Salt Bridge
- A tube filled with an electrolyte (e.g., sodium chloride) connecting the two solutions.
- Prevents a buildup of charge in each half-cell by allowing ions to flow between the solutions.
- Positive ions from the salt bridge move toward the negative side to balance charge.
- Negative ions from the salt bridge move toward the positive side to balance charge.
Overall Changes in the Voltaic Cell
- The zinc metal dissolves as atoms lose electrons and become ions in the solution.
- The copper metal increases in size as copper ions gain electrons and become neutral atoms that attach to the metal.
- The flow of electrons through the wire constitutes the electric current generated by the voltaic cell.
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Description
Test your knowledge on voltaic cells and their operation. This quiz covers the chemical reactions involved, the setup of a basic voltaic cell, and the movement of electrons within the system. Challenge yourself to understand the principles that generate electricity from chemical reactions.
