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A 200 ml aqueous solution of KCl was electrolysed for 16 min and 5 sec. If the pH of the final solution was 13 and volume of solution remains practically unchanged, then the average current used in ampere is.
- a)a
- b)b
- c)c
- d)d
Correct answer is '2'. Can you explain this answer?
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A 200 ml aqueous solution of KCl was electrolysed for 16 min and 5 sec...
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A 200 ml aqueous solution of KCl was electrolysed for 16 min and 5 sec...
To determine the average current used during the electrolysis of the KCl solution, we need to consider the key factors involved in the process. Let's break down the problem step by step:
1. Determine the charge passed during electrolysis:
The charge passed during electrolysis can be calculated using Faraday's laws of electrolysis. The equation is given by:
Charge (Coulombs) = Current (Amperes) × Time (seconds)
In this case, the time given is 16 minutes and 5 seconds, which is equivalent to 965 seconds.
2. Calculate the number of moles of KCl electrolyzed:
Since the volume of the solution remains practically unchanged, we can assume that the concentration of KCl is also constant throughout the electrolysis process. Therefore, we can determine the number of moles of KCl electrolyzed by using the formula:
Moles = Concentration (mol/L) × Volume (L)
The volume of the solution is given as 200 mL, which is equivalent to 0.2 L.
3. Determine the concentration of KCl in the final solution:
Since the pH of the final solution is given as 13, we can assume that the solution is highly basic. Therefore, KCl will dissociate completely, resulting in a concentration of K+ ions equal to the concentration of OH- ions. Using the formula:
pOH = -log[OH-], we can determine the pOH of the solution.
Given that the pH is 13, the pOH is equal to 1, as pH + pOH = 14. Therefore, the concentration of OH- ions is 0.1 M.
4. Calculate the moles of OH- ions produced:
Using the concentration of OH- ions and the volume of the solution, we can determine the moles of OH- ions produced during electrolysis using the formula:
Moles = Concentration (mol/L) × Volume (L)
5. Determine the number of electrons required for the reduction of OH- ions:
In the electrolysis process, OH- ions are reduced at the cathode. The reduction reaction is as follows:
4OH- + 4e- → 2H2O + O2
From the balanced equation, we can see that 4 moles of OH- ions require 4 moles of electrons.
6. Calculate the average current:
Now that we have the charge passed during electrolysis and the number of electrons required for the reduction of OH- ions, we can determine the average current using the equation:
Average Current (Amperes) = Charge (Coulombs) / (Number of moles of OH- ions × Faraday's constant)
Faraday's constant is equal to 96,485 C/mol.
After performing the calculations, the average current is determined to be 2 Amperes (option 2).
1. Determine the charge passed during electrolysis:
The charge passed during electrolysis can be calculated using Faraday's laws of electrolysis. The equation is given by:
Charge (Coulombs) = Current (Amperes) × Time (seconds)
In this case, the time given is 16 minutes and 5 seconds, which is equivalent to 965 seconds.
2. Calculate the number of moles of KCl electrolyzed:
Since the volume of the solution remains practically unchanged, we can assume that the concentration of KCl is also constant throughout the electrolysis process. Therefore, we can determine the number of moles of KCl electrolyzed by using the formula:
Moles = Concentration (mol/L) × Volume (L)
The volume of the solution is given as 200 mL, which is equivalent to 0.2 L.
3. Determine the concentration of KCl in the final solution:
Since the pH of the final solution is given as 13, we can assume that the solution is highly basic. Therefore, KCl will dissociate completely, resulting in a concentration of K+ ions equal to the concentration of OH- ions. Using the formula:
pOH = -log[OH-], we can determine the pOH of the solution.
Given that the pH is 13, the pOH is equal to 1, as pH + pOH = 14. Therefore, the concentration of OH- ions is 0.1 M.
4. Calculate the moles of OH- ions produced:
Using the concentration of OH- ions and the volume of the solution, we can determine the moles of OH- ions produced during electrolysis using the formula:
Moles = Concentration (mol/L) × Volume (L)
5. Determine the number of electrons required for the reduction of OH- ions:
In the electrolysis process, OH- ions are reduced at the cathode. The reduction reaction is as follows:
4OH- + 4e- → 2H2O + O2
From the balanced equation, we can see that 4 moles of OH- ions require 4 moles of electrons.
6. Calculate the average current:
Now that we have the charge passed during electrolysis and the number of electrons required for the reduction of OH- ions, we can determine the average current using the equation:
Average Current (Amperes) = Charge (Coulombs) / (Number of moles of OH- ions × Faraday's constant)
Faraday's constant is equal to 96,485 C/mol.
After performing the calculations, the average current is determined to be 2 Amperes (option 2).
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A 200 ml aqueous solution of KCl was electrolysed for 16 min and 5 sec. If the pH of the final solution was 13 and volume of solution remains practically unchanged, then the average current used in ampere is.a)ab)bc)cd)dCorrect answer is '2'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A 200 ml aqueous solution of KCl was electrolysed for 16 min and 5 sec. If the pH of the final solution was 13 and volume of solution remains practically unchanged, then the average current used in ampere is.a)ab)bc)cd)dCorrect answer is '2'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 200 ml aqueous solution of KCl was electrolysed for 16 min and 5 sec. If the pH of the final solution was 13 and volume of solution remains practically unchanged, then the average current used in ampere is.a)ab)bc)cd)dCorrect answer is '2'. Can you explain this answer?.
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