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If 4.59 A is applied for 68 minutes, what mass of Pb(s) will be produced? g Pb

If 4.59 A is applied for 68 minutes, what mass of Pb(s) will be produced? g Pb

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
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**Question:** If 4.59 A is applied for 68 minutes, what mass of Pb(s) will be produced? **Answer:** [Blank field] g Pb
Transcribed Image Text:**Question:** If 4.59 A is applied for 68 minutes, what mass of Pb(s) will be produced? **Answer:** [Blank field] g Pb
The diagram illustrates the process of electrolysis of molten lead(II) chloride (PbCl₂). Here's a detailed explanation of the components and process depicted: 1. **Molten PbCl₂**: The container holds molten lead(II) chloride, which serves as the electrolyte for the electrolysis process. 2. **Electrodes**: There are two electrodes immersed in the molten PbCl₂: - **Anode**: The positively charged electrode where oxidation occurs. Electrons are withdrawn from ions in the electrolyte, causing them to be oxidized. - **Cathode**: The negatively charged electrode where reduction occurs. Electrons are supplied to ions in the electrolyte, causing them to be reduced. 3. **Voltage Source**: This provides the electric current necessary for the electrolysis. The current flows from the anode to the cathode, driven by the potential difference. 4. **Porous Screen**: Positioned between the anode and cathode, the porous screen prevents the products of electrolysis from mixing back into the electrolyte, ensuring efficient separation of the resulting substances. 5. **Flow of Electrons (e⁻)**: The diagram shows electrons moving towards the anode and away from the cathode, indicating oxidation at the anode and reduction at the cathode. In summary, the setup is used to decompose molten lead(II) chloride into its constituent elements through the application of electrical energy. The anode attracts chloride ions, leading to the formation of chlorine gas, while the cathode attracts lead ions, resulting in the deposition of molten lead.
Transcribed Image Text:The diagram illustrates the process of electrolysis of molten lead(II) chloride (PbCl₂). Here's a detailed explanation of the components and process depicted: 1. **Molten PbCl₂**: The container holds molten lead(II) chloride, which serves as the electrolyte for the electrolysis process. 2. **Electrodes**: There are two electrodes immersed in the molten PbCl₂: - **Anode**: The positively charged electrode where oxidation occurs. Electrons are withdrawn from ions in the electrolyte, causing them to be oxidized. - **Cathode**: The negatively charged electrode where reduction occurs. Electrons are supplied to ions in the electrolyte, causing them to be reduced. 3. **Voltage Source**: This provides the electric current necessary for the electrolysis. The current flows from the anode to the cathode, driven by the potential difference. 4. **Porous Screen**: Positioned between the anode and cathode, the porous screen prevents the products of electrolysis from mixing back into the electrolyte, ensuring efficient separation of the resulting substances. 5. **Flow of Electrons (e⁻)**: The diagram shows electrons moving towards the anode and away from the cathode, indicating oxidation at the anode and reduction at the cathode. In summary, the setup is used to decompose molten lead(II) chloride into its constituent elements through the application of electrical energy. The anode attracts chloride ions, leading to the formation of chlorine gas, while the cathode attracts lead ions, resulting in the deposition of molten lead.
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