Question
Use the reactions to complete the activity.
Zn+CuSO4→ZnSO4+Cu
Zinc (Zn) reacts with copper sulfate (CuSO4) to form zinc sulfate (ZnSO4) and copper (Cu). A classmate tells you this is a reaction in a galvanic cell. Describe how you know your classmate is correct?
Zn+CuSO4→ZnSO4+Cu
Zinc (Zn) reacts with copper sulfate (CuSO4) to form zinc sulfate (ZnSO4) and copper (Cu). A classmate tells you this is a reaction in a galvanic cell. Describe how you know your classmate is correct?
Answers
Answered by
GPT-4o mini
Your classmate is correct in identifying the reaction between zinc (Zn) and copper sulfate (CuSO4) as a reaction that can occur in a galvanic cell. Here are some key points that support this conclusion:
1. **Redox Reaction**: The reaction involves the transfer of electrons between zinc and copper ions, which is characteristic of a redox (reduction-oxidation) reaction. Zinc is oxidized as it loses electrons, and copper ions are reduced as they gain electrons.
2. **Electrode Materials**: In a galvanic cell, one metal serves as the anode (the site of oxidation) and another as the cathode (the site of reduction). In this case, zinc would serve as the anode where zinc is oxidized to Zn²⁺, and copper serves as the cathode where Cu²⁺ ions from the copper sulfate solution are reduced to solid copper.
3. **Spontaneous Reaction**: The reaction is spontaneous under standard conditions. In a galvanic cell, spontaneous reactions generate electrical energy as electrons flow from the anode to the cathode.
4. **Electron Flow**: The oxidation of zinc releases electrons, which flow through an external circuit to the copper cathode. This flow of electrons can be harnessed to do work, which is a key feature of galvanic cells.
5. **Ion Migration**: In a galvanic cell, ions in the electrolyte (Cu²⁺ in this case) migrate toward the electrodes where they undergo reduction, consistent with the behavior seen in this reaction.
Overall, the characteristics of the reaction align well with the principles of galvanic cells, demonstrating that your classmate's assertion is indeed accurate.
1. **Redox Reaction**: The reaction involves the transfer of electrons between zinc and copper ions, which is characteristic of a redox (reduction-oxidation) reaction. Zinc is oxidized as it loses electrons, and copper ions are reduced as they gain electrons.
2. **Electrode Materials**: In a galvanic cell, one metal serves as the anode (the site of oxidation) and another as the cathode (the site of reduction). In this case, zinc would serve as the anode where zinc is oxidized to Zn²⁺, and copper serves as the cathode where Cu²⁺ ions from the copper sulfate solution are reduced to solid copper.
3. **Spontaneous Reaction**: The reaction is spontaneous under standard conditions. In a galvanic cell, spontaneous reactions generate electrical energy as electrons flow from the anode to the cathode.
4. **Electron Flow**: The oxidation of zinc releases electrons, which flow through an external circuit to the copper cathode. This flow of electrons can be harnessed to do work, which is a key feature of galvanic cells.
5. **Ion Migration**: In a galvanic cell, ions in the electrolyte (Cu²⁺ in this case) migrate toward the electrodes where they undergo reduction, consistent with the behavior seen in this reaction.
Overall, the characteristics of the reaction align well with the principles of galvanic cells, demonstrating that your classmate's assertion is indeed accurate.
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