Question

calculate the moles of copper metal that can be produced by the electrolysis of molten copper sulphate using 500c of electricity​

Answer 1

Explanation:

Calculate the moles of copper metal that can be produced by the electrolysis of molten copper sulfate using 500 C of electricity. 5.

...

Extract the data from the question: Q = ? C. n(e-) = 2 mol. F = 96,500 C mol-1.

Write the equation: Q = n(e-) x F.

Substitute the values into the equation and solve:

Answer 2

Given:

Charge= 500C

Electrolysis reaction: CuSO₄ ⇄ Cu²⁺ + SO₄²⁻

                                    Cu²⁺ + 2e⁻ → Cu (s)

To find:

The moles of copper metal produced

Solution:

The question can be solved using Faraday's law of electrolysis which states that “The mass of a substance deposited at any electrode is directly proportional to the amount of charge passed.”

We know that 1F = 96500C

So, 500C = $\frac{1}{96500} X 500$F

According to the chemical equation,

2F of charge is needed to deposit 1 mole of copper metal.

or 2F charge deposits 63.5g Cu

So, 1/965 F will deposit  $\frac{63.5}{965 X 2}$

= 0.032g

Number of moles= $\frac{Given Mass}{Molar Mass}$

= 0.032/63.5

=5 x 10⁻⁴ moles

Hence, 5 x 10⁻⁴ moles of copper are produced.