salt bridge Mg Ag N Mg(NO₂)₂ AgNO, If the cell pictured above is driven as an electrolytic cell: The electrons would flow [Select] The standard (assuming 1 M concentrations) cell potential i ✔ [Select] -1.56 V +1.56 V +3.16 V -3.16 V The following statement is true: [Select] If the salt bridge contains KCI, then [Select] In order to decrease (make it a smaller number) the potential necessary for electrolysis, [Select] If the current is set to a constant of 5.37 A for 5.00 min. then [Select] Question 4 Voltmeter V of metal would deposit on the catho-
salt bridge Mg Ag N Mg(NO₂)₂ AgNO, If the cell pictured above is driven as an electrolytic cell: The electrons would flow [Select] The standard (assuming 1 M concentrations) cell potential i ✔ [Select] -1.56 V +1.56 V +3.16 V -3.16 V The following statement is true: [Select] If the salt bridge contains KCI, then [Select] In order to decrease (make it a smaller number) the potential necessary for electrolysis, [Select] If the current is set to a constant of 5.37 A for 5.00 min. then [Select] Question 4 Voltmeter V of metal would deposit on the catho-
Transcribed Image Text:**Question 3: Electrochemistry Problem**
The image displays an electrochemical cell setup with two electrodes: magnesium (Mg) and silver (Ag). The Mg electrode is immersed in a solution of Mg(NO₃)₂, and the Ag electrode is immersed in a solution of AgNO₃. A salt bridge connects the two solutions, allowing the flow of ions, and a voltage source is applied across the electrodes.
**Diagram Explanation:**
- **Voltage Source:** Indicates the direction of electron flow through the external circuit.
- **Mg Electrode:** Connected to a solution of magnesium nitrate (Mg(NO₃)₂).
- **Ag Electrode:** Connected to a solution of silver nitrate (AgNO₃).
- **Salt Bridge:** Allows for ion migration to maintain electrical neutrality.
**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.
This setup can be used to explore the principles of electrolysis and electrochemical cell reactions, with focus on electrode potentials, ion movement, and deposition rates.
Transcribed Image Text:### Diagram Explanation
The diagram illustrates an electrolytic cell setup with a voltage source connected to two electrodes: magnesium (Mg) and silver (Ag). Each electrode is immersed in a solution: magnesium nitrate \((\text{Mg(NO}_3\text{)}_2)\) and silver nitrate \((\text{AgNO}_3)\). A salt bridge connects the two solutions, facilitating ion flow to complete the circuit.
### Instructions for Problem Solving
**1. Electron Flow in Electrolytic Cell:**
- If the cell is driven as an electrolytic cell, determine the direction for electron flow.
**2. Standard Cell Potential:**
- Choose the standard cell potential assuming 1 M concentrations from the options:
- -1.56 V
- +1.56 V
- +3.16 V
- -3.16 V
**3. True Statement Verification:**
- Confirm which statement is true using the available options.
**4. Effect of KCl in Salt Bridge:**
- State the effect if the salt bridge contains KCl.
**5. Decrease in Electrolysis Potential:**
- Select the method to decrease the potential necessary for electrolysis.
**6. Metal Deposition Calculation:**
- Calculate the amount of metal deposited on the cathode if the current is set at 5.37 A for 5.00 minutes.
### Additional Instructions
- Analyze and solve each question based on standard electrochemical principles.
- Make sure to apply Faraday’s laws of electrolysis for calculating metal deposition.
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![**Question 3: Electrochemistry Problem**
The image displays an electrochemical cell setup with two electrodes: magnesium (Mg) and silver (Ag). The Mg electrode is immersed in a solution of Mg(NO₃)₂, and the Ag electrode is immersed in a solution of AgNO₃. A salt bridge connects the two solutions, allowing the flow of ions, and a voltage source is applied across the electrodes.
**Diagram Explanation:**
- **Voltage Source:** Indicates the direction of electron flow through the external circuit.
- **Mg Electrode:** Connected to a solution of magnesium nitrate (Mg(NO₃)₂).
- **Ag Electrode:** Connected to a solution of silver nitrate (AgNO₃).
- **Salt Bridge:** Allows for ion migration to maintain electrical neutrality.
**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.
This setup can be used to explore the principles of electrolysis and electrochemical cell reactions, with focus on electrode potentials, ion movement, and deposition rates.](https://content.bartleby.com/qna-images/question/f3a38996-6782-40c2-af9f-f624a7021da3/50c765c3-9292-44a0-9c2a-ce57725cb9f1/ljipy2_processed.jpeg)
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