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Question: 10g fairly concentrated solution of \(CuS{O_4}\) is electrolysed using 0.01 faraday of electricity. ...

10g fairly concentrated solution of CuSO4CuS{O_4} is electrolysed using 0.01 faraday of electricity. Calculate the mass of the resulting solution.
a.) 7.6025g
b.) 9.6025g
c.) 6.6025g
d.) 77.6025g

Explanation

Solution

In order to deal with this question first we will write the reaction of the given compound then we will proceed further by applying Faraday's law so that we will get 1 faraday current and by substituting the obtained mass with initial mass we will get the required answer.
Formula used- W=ZQW = ZQ, where Q=I×t=current×timeQ = I \times t = current \times time

Complete step by step answer:
Given that the Initial solution weight is 10g.
Reaction formed:
At anode: Cu+2+2e−→CuC{u^{ + 2}} + 2{e^ - } \to Cu

At cathode: 2H2O→4H++O2+4e−2{H_2}O \to 4{H^ + } + {O_2} + 4{e^ - }
According to Faraday's law,
W=ZQW = ZQ,
And Q=I×t=current×timeQ = I \times t = current \times time
Where Z is electrochemical equivalent
And W is the weight of the substance
From the given equations we have:
So, 1 faraday deposits 0.5 mole of Cu.
1 faraday current deposit 63.52g=31.75g\dfrac{{63.5}}{2}g = 31.75g of copper
So, 0.01 faraday current deposit 31.75×0.01=0.3175g31.75 \times 0.01 = 0.3175gof copper
Initial solution weight is 10g.
Therefore, after electrolysis weight of the solution is 10g−0.3175g=9.6825g≈9.6025g10g - 0.3175g = 9.6825g \approx 9.6025g
Hence the mass of the resulting solution is 9.6025g
So, the correct answer is “Option B”.

Additional Information:
Copper sulphate is used in both agricultural and non-agricultural environments as a fungicide, algaecide, root-killer and herbicide. This is used also as an antimicrobial and molluscicide. Uses for individual copper-sulphate products differ greatly.

Note: Electrolysis, method of passing electrical current through a material to induce a chemical transition. The chemical transition is one where the material loses an electron (oxidation or reduction) or retains one. The procedure is carried out in an electrolytic cell, a device composed of positive and negative electrodes isolated and dipped into a solution containing ions that are charged positively and negatively. The material to be converted may represent the electrode, may be the solution, or may be dissolved in the solution.