Mg Mg(NO₂) salt bridge If the cell pictured above is driven as an electrolytic cell: The electrons would flow [Select] me following statement is true: [Select] The standard (assuming 1 M concentrations) cell potential is [Select) the salt bridge contains KCL, then [Select] estion 4 Ag AgNO, order to decrease (make it a smaller number) the potential necessary for electrolysis, [Select] me current is set to a constant of 5.37 A for 5.00 min. the Voltmeter [Select] 0.406 g 0.203 g 0.901 g 0.00338 of metal would deposit on the cathode.

Chemistry
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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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Electrochemical Cell Experiment

#### Diagram Explanation

The image depicts a diagram of an electrochemical cell. The setup includes:

- **Two Electrodes**: Magnesium (Mg) and Silver (Ag), each placed in their respective solutions, Mg(NO\(_3\))\(_2\) and AgNO\(_3\).
- **Salt Bridge**: A U-shaped tube that connects the two solutions to maintain electrical neutrality by allowing the flow of ions.
- **Voltmeter**: Connected in the circuit to measure the potential difference between the electrodes.

#### Interactive Questions

The following statements pertain to the experimental setup:

1. **Electrons Flow Direction**: [Select]
   - Options involve choosing the direction in which electrons would flow in the circuit.

2. **Standard Cell Potential**: [Select]
   - The standard cell potential is determined under standard conditions.

3. **True Statements**: [Select]
   - Evaluate specific statements about the cell and select the accurate one.

4. **Effect of KCl in Salt Bridge**: [Select]
   - Determines what happens when the salt bridge contains KCl.

5. **Necessary Potential for Electrolysis**: [Select]
   - The potential needed for electrolysis could vary based on changes to the system.

6. **Mass Deposition Calculation**
   - When the current is constant at 5.37 A for 5.00 minutes, calculate the mass of metal deposited on the cathode:
     - Options: 
       - 0.406 g
       - 0.203 g
       - 0.901 g
       - 0.00338 g

This interactive exercise helps students understand the principles of electrochemistry, including electron flow, cell potential, and the impact of altering conditions on metal deposition.
Transcribed Image Text:### Electrochemical Cell Experiment #### Diagram Explanation The image depicts a diagram of an electrochemical cell. The setup includes: - **Two Electrodes**: Magnesium (Mg) and Silver (Ag), each placed in their respective solutions, Mg(NO\(_3\))\(_2\) and AgNO\(_3\). - **Salt Bridge**: A U-shaped tube that connects the two solutions to maintain electrical neutrality by allowing the flow of ions. - **Voltmeter**: Connected in the circuit to measure the potential difference between the electrodes. #### Interactive Questions The following statements pertain to the experimental setup: 1. **Electrons Flow Direction**: [Select] - Options involve choosing the direction in which electrons would flow in the circuit. 2. **Standard Cell Potential**: [Select] - The standard cell potential is determined under standard conditions. 3. **True Statements**: [Select] - Evaluate specific statements about the cell and select the accurate one. 4. **Effect of KCl in Salt Bridge**: [Select] - Determines what happens when the salt bridge contains KCl. 5. **Necessary Potential for Electrolysis**: [Select] - The potential needed for electrolysis could vary based on changes to the system. 6. **Mass Deposition Calculation** - When the current is constant at 5.37 A for 5.00 minutes, calculate the mass of metal deposited on the cathode: - Options: - 0.406 g - 0.203 g - 0.901 g - 0.00338 g This interactive exercise helps students understand the principles of electrochemistry, including electron flow, cell potential, and the impact of altering conditions on metal deposition.
### Question 3

**Diagram Description:**
The diagram illustrates an electrolytic cell setup with a voltage source. The cell includes a salt bridge connecting two solutions: magnesium nitrate (Mg(NO₃)₂) on one side with a magnesium (Mg) electrode, and silver nitrate (AgNO₃) on the other side with a silver (Ag) electrode.

**Questions:**

1. If the cell pictured above is driven as an electrolytic cell:
   - The electrons would flow [Select]

2. The standard (assuming 1 M concentrations) cell potential is:
   - -1.56 V [Select]

3. The following statement is true:
   - [Select]

4. If the salt bridge contains KCl, then:
   - [Select]

5. In order to decrease (make it a smaller number) the potential necessary for electrolysis:
   - [Select]

6. If the current is set to a constant of 5.37 A for 5.00 min, then:
   - [Select] of metal would deposit on the cathode.
Transcribed Image Text:### Question 3 **Diagram Description:** The diagram illustrates an electrolytic cell setup with a voltage source. The cell includes a salt bridge connecting two solutions: magnesium nitrate (Mg(NO₃)₂) on one side with a magnesium (Mg) electrode, and silver nitrate (AgNO₃) on the other side with a silver (Ag) electrode. **Questions:** 1. If the cell pictured above is driven as an electrolytic cell: - The electrons would flow [Select] 2. The standard (assuming 1 M concentrations) cell potential is: - -1.56 V [Select] 3. The following statement is true: - [Select] 4. If the salt bridge contains KCl, then: - [Select] 5. In order to decrease (make it a smaller number) the potential necessary for electrolysis: - [Select] 6. If the current is set to a constant of 5.37 A for 5.00 min, then: - [Select] of metal would deposit on the cathode.
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