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On passing a current of 1.0 ampere for 16 min and 5 sec through one litre solution of CuCl2, all copper of the solution was deposited at cathode. The strength of CuCl2 solution was (Molar mass of Cu= 63.5; Faraday constant = 96,500 Cmol–1) [1996]
  • a)
    0.01 N
  • b)
    0.01 M
  • c)
    0.02 M
  • d)
    0.2 N
Correct answer is option 'A'. Can you explain this answer?
Verified Answer
On passing a current of 1.0 ampere for 16 min and 5 sec through one li...
By Faraday's Ist Law, 
(where q = it = charge of ion) we know that no of equivalent
(where i= 1 A, t = 16×60+5 = 965 sec.) Since, we know that
Normality 
= 0.01 N
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Most Upvoted Answer
On passing a current of 1.0 ampere for 16 min and 5 sec through one li...
-1)

First, we need to calculate the amount of charge that passed through the solution:

Q = It = (1.0 A)(16 min 5 sec) = 965 C

Next, we can use Faraday's law of electrolysis to relate the amount of charge to the amount of copper deposited:

n = Q/F

where n is the number of moles of copper deposited, Q is the amount of charge passed through the solution, and F is Faraday's constant.

n = (965 C) / (96,500 C/mol) = 0.01 mol

Since we started with 1 litre of solution, the concentration of CuCl2 can be calculated as follows:

0.01 mol / 1 L = 0.01 M

Finally, we need to take into account that CuCl2 dissociates into Cu2+ and 2Cl- ions in solution. Therefore, the actual concentration of CuCl2 in the solution is twice the concentration of Cu2+ ions:

[CuCl2] = 0.01 M / 2 = 0.005 M

Therefore, the strength of the CuCl2 solution is 0.005 M.
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On passing a current of 1.0 ampere for 16 min and 5 sec through one litre solution of CuCl2, all copper of the solution was deposited at cathode. The strength of CuCl2 solution was (Molar mass of Cu= 63.5; Faraday constant = 96,500 Cmol–1) [1996]a)0.01 Nb)0.01 Mc)0.02 Md)0.2 NCorrect answer is option 'A'. Can you explain this answer?
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On passing a current of 1.0 ampere for 16 min and 5 sec through one litre solution of CuCl2, all copper of the solution was deposited at cathode. The strength of CuCl2 solution was (Molar mass of Cu= 63.5; Faraday constant = 96,500 Cmol–1) [1996]a)0.01 Nb)0.01 Mc)0.02 Md)0.2 NCorrect answer is option 'A'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about On passing a current of 1.0 ampere for 16 min and 5 sec through one litre solution of CuCl2, all copper of the solution was deposited at cathode. The strength of CuCl2 solution was (Molar mass of Cu= 63.5; Faraday constant = 96,500 Cmol–1) [1996]a)0.01 Nb)0.01 Mc)0.02 Md)0.2 NCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for On passing a current of 1.0 ampere for 16 min and 5 sec through one litre solution of CuCl2, all copper of the solution was deposited at cathode. The strength of CuCl2 solution was (Molar mass of Cu= 63.5; Faraday constant = 96,500 Cmol–1) [1996]a)0.01 Nb)0.01 Mc)0.02 Md)0.2 NCorrect answer is option 'A'. Can you explain this answer?.
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