Electrolysis Copper(II) Nitrate: Silver & Gold Impurities

[AryaUnderfoot]

Homework Statement

Electrolysis of an aqueous solution of copper(II) nitrate was carried out using copper electrodes. The mass of the anode decreased by 1.28 g while that of the cathode increased by 1.18 g
Assuming that the copper anode contains silver and gold impurities, which statement is true?
A. The blue colour of aqueous solution of copper(II) nitrate become darker
B. 0.10 g of silver and gold were collected from the electrolysis
C. The quantity of electricity used was 1790C
D. 1.28 g of copper dissolved at the anode

Homework Equations

The Attempt at a Solution

A and D should be wrong because the mass of copper dissolved at anode is lower than the mass of copper deposits at cathode
While for C, Cu²⁺+2e-->Cu
2F = 1 mol of Cu
x = 1.18/63.5 mol of Cu
Therfore, x= 3586C
So C should be wrong. But the answer is C
As for B, I don't have a clue

 

[Borek]

the mass of copper dissolved at anode is lower than the mass of copper deposits at cathode

You don't know that - assuming the anode made of pure copper more could dissolved than deposited. However, if it were only 50% copper less dissolved than deposited. So all we can say is that we don't know whether the amount of copper in the solution changed - and that eliminates A, B and D, but for a different reason than you thought,

You are right about the charge required being 3.59×10³ C, apparently whoever wrote the question forgot about factor of 2 (as the answer given is exactly half of the correct one).

 

[epenguin]

apparently whoever wrote the question forgot about factor of 2 (as the answer given is exactly half of the correct one).

He writes a lot of the questions here.