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Chapter 7: Problem 44

Assertion (A): Passage of 48,250 coulombs of electricity through cupric sulphate and ferrous sulphate solutions result in the deposition \(0.5\) moles each of iron and copper at the respective cathodes. Reason (R): Number of equivalents of a metal deposited at cathode is equal to the number of faradays of electricity passed through the electrolyte. (a) Both "A" and "R" are true and "R" is the correct explanation of "A". (b) Both "A" and "R" are true and "R" is not the correct explanation of "A". (c) "A" is correct and "R" is wrong. (d) "A" is wrong and "R" is correct.

Short Answer

Expert verified
Explain your answer using Faraday's laws of electrolysis. Answer: No, the passage of 48,250 coulombs of electricity results in the deposition of 0.25 moles each of iron and copper at the respective cathodes, not 0.5 moles. This is determined using Faraday's laws of electrolysis, which states that the number of equivalents of a metal deposited at the cathode is equal to the number of faradays of electricity passed through the electrolyte.

Step by step solution

01

Analyze Assertion (A)

First, we need to determine if the passage of 48,250 coulombs of electricity through cupric sulfate and ferrous sulfate solutions result in the deposition of 0.5 moles each of iron and copper at the respective cathodes. Copper (Cu) has a valency of +2, and hence its equivalent weight is atomic mass / 2 = 63.5 / 2. Iron (Fe) also has a valency of +2, and its equivalent weight is atomic mass / 2 = 55.8 / 2. Using Faraday's Law, we know that the number of equivalents = charge passed (in coulombs) / (n * Faraday's constant), where n is the valency of the metal. Faraday's constant is approximately 96,500 C/mol.
02

Calculate the number of equivalents of Cu and Fe deposited on the respective cathodes

For copper: Number of equivalents of Cu = Charge passed / (2 * 96,500) = 48,250 / (2 * 96,500) = 0.25 mol For iron: Number of equivalents of Fe = Charge passed / (2 * 96,500) = 48,250 / (2 * 96,500) = 0.25 mol Since we have calculated the number of moles of each metal deposited at the cathodes and it doesn't match the amount stated in Assertion (A), we can conclude that Assertion (A) is incorrect.
03

Analyze Reason (R)

Now let's analyze the Reason (R). The statement says that "Number of equivalents of a metal deposited at cathode is equal to the number of faradays of electricity passed through the electrolyte." This statement describes Faraday's Law of electrolysis and it's correct. According to Faraday's law, the amount of substance transformed in an electrolytic cell is proportional to the amount of electrical charge passed through the cell.
04

Determine the relationship between "A" and "R"

Now we have the conclusions about Assertion (A) and Reason (R). 1. Assertion (A) is incorrect, as the passage of 48,250 coulombs of electricity will not result in the deposition of 0.5 moles each of iron and copper at the respective cathodes, but instead 0.25 moles each. 2. Reason (R) is correct, as it accurately describes Faraday's Law of electrolysis. Therefore, the correct answer is (d) "A" is wrong and "R" is correct.

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Most popular questions from this chapter

Ratio of number of Faradays of electricity required to deposit magnesium, aluminium and sodium in equimolar ratio on electrolysis of their respective molten salts is (a) \(2: 3: 2\) (b) \(2: 1: 1\) (c) \(2: 3: 1\) (d) \(4: 6: 1\)

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