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The electrochemical cell shown below is a concentration cell. M | M2+ (saturated solution of a sparingly soluble salt, MX2) | | M2+ (0.001 mol dm-3) |M The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059 V.
Q.
The value of ΔG (kJ mol-1) for the given cell is (take 1 F= 96500 C mol-1)
- a)-5.7
- b)5.7
- c)11.4
- d)-11.4
Correct answer is option 'D'. Can you explain this answer?
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The electrochemical cell shown below is a concentration cell. M |M2+ (...
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The electrochemical cell shown below is a concentration cell. M |M2+ (...
Given Information:
- The electrochemical cell is a concentration cell.
- The cell consists of two electrodes: M and M2.
- The M electrode is in contact with a saturated solution of a sparingly soluble salt, MX2.
- The M2 electrode is in contact with a 0.001 mol dm-3 solution of M2 ions.
- The emf of the cell at 298K is 0.059 V.
Explanation:
To determine the value of G (kJ mol-1) for the given cell, we can use the equation:
ΔG = -nFE
where ΔG is the change in Gibbs free energy, n is the number of moles of electrons transferred, F is the Faraday constant (1 F = 96500 C mol-1), and E is the emf of the cell.
Step 1: Finding the number of moles of electrons transferred (n):
In a concentration cell, no redox reaction takes place. Therefore, the number of moles of electrons transferred (n) is zero.
Step 2: Calculating the value of ΔG:
Since n is zero, the equation simplifies to:
ΔG = 0
Therefore, the value of ΔG for the given cell is zero.
Step 3: Converting ΔG to kJ mol-1:
Since ΔG is zero, the value of ΔG in kJ mol-1 is also zero.
Conclusion:
The value of G (kJ mol-1) for the given cell is 0 kJ mol-1. Therefore, the correct answer is option 'D' (-11.4 kJ mol-1).
- The electrochemical cell is a concentration cell.
- The cell consists of two electrodes: M and M2.
- The M electrode is in contact with a saturated solution of a sparingly soluble salt, MX2.
- The M2 electrode is in contact with a 0.001 mol dm-3 solution of M2 ions.
- The emf of the cell at 298K is 0.059 V.
Explanation:
To determine the value of G (kJ mol-1) for the given cell, we can use the equation:
ΔG = -nFE
where ΔG is the change in Gibbs free energy, n is the number of moles of electrons transferred, F is the Faraday constant (1 F = 96500 C mol-1), and E is the emf of the cell.
Step 1: Finding the number of moles of electrons transferred (n):
In a concentration cell, no redox reaction takes place. Therefore, the number of moles of electrons transferred (n) is zero.
Step 2: Calculating the value of ΔG:
Since n is zero, the equation simplifies to:
ΔG = 0
Therefore, the value of ΔG for the given cell is zero.
Step 3: Converting ΔG to kJ mol-1:
Since ΔG is zero, the value of ΔG in kJ mol-1 is also zero.
Conclusion:
The value of G (kJ mol-1) for the given cell is 0 kJ mol-1. Therefore, the correct answer is option 'D' (-11.4 kJ mol-1).
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The electrochemical cell shown below is a concentration cell. M |M2+ (saturated solution of a sparingly soluble salt, MX2) ||M2+(0.001 mol dm-3) |M The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059 V.Q.The value of G (kJ mol-1) for the given cell is (take 1 F= 96500 C mol-1)a)-5.7b)5.7c)11.4d)-11.4Correct answer is option 'D'. Can you explain this answer?
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The electrochemical cell shown below is a concentration cell. M |M2+ (saturated solution of a sparingly soluble salt, MX2) ||M2+(0.001 mol dm-3) |M The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059 V.Q.The value of G (kJ mol-1) for the given cell is (take 1 F= 96500 C mol-1)a)-5.7b)5.7c)11.4d)-11.4Correct answer is option 'D'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The electrochemical cell shown below is a concentration cell. M |M2+ (saturated solution of a sparingly soluble salt, MX2) ||M2+(0.001 mol dm-3) |M The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059 V.Q.The value of G (kJ mol-1) for the given cell is (take 1 F= 96500 C mol-1)a)-5.7b)5.7c)11.4d)-11.4Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The electrochemical cell shown below is a concentration cell. M |M2+ (saturated solution of a sparingly soluble salt, MX2) ||M2+(0.001 mol dm-3) |M The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059 V.Q.The value of G (kJ mol-1) for the given cell is (take 1 F= 96500 C mol-1)a)-5.7b)5.7c)11.4d)-11.4Correct answer is option 'D'. Can you explain this answer?.
The electrochemical cell shown below is a concentration cell. M |M2+ (saturated solution of a sparingly soluble salt, MX2) ||M2+(0.001 mol dm-3) |M The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059 V.Q.The value of G (kJ mol-1) for the given cell is (take 1 F= 96500 C mol-1)a)-5.7b)5.7c)11.4d)-11.4Correct answer is option 'D'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The electrochemical cell shown below is a concentration cell. M |M2+ (saturated solution of a sparingly soluble salt, MX2) ||M2+(0.001 mol dm-3) |M The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059 V.Q.The value of G (kJ mol-1) for the given cell is (take 1 F= 96500 C mol-1)a)-5.7b)5.7c)11.4d)-11.4Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The electrochemical cell shown below is a concentration cell. M |M2+ (saturated solution of a sparingly soluble salt, MX2) ||M2+(0.001 mol dm-3) |M The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298K is 0.059 V.Q.The value of G (kJ mol-1) for the given cell is (take 1 F= 96500 C mol-1)a)-5.7b)5.7c)11.4d)-11.4Correct answer is option 'D'. Can you explain this answer?.
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