A current of 19296 C is passed through an aqueous solution of copper sulphate using copper electrodes. What is the mass (in g ) of copper deposited at the cathode? (Molar mass of Cu =63.5 g mol -1 )

Question

A current of 19296 C is passed through an aqueous solution of copper sulphate using copper electrodes. What is the mass (in g ) of copper deposited at the cathode? (Molar mass of Cu =63.5 g mol -1 ) (A) 3.17 (B) 1.58 (C) 6.35 (D) 0.79

Tardigrade Admin · Accepted Answer

Given, Charge used =19296 C Molar mass of Cu =63.5 ∵ Cu in CuSO 4 has Cu 2+ charge means: 2 × 96500 C of charge give =63.5 g of Cu Thus, 19296 C of charge give =(63.5 × 19296/2 × 96500) =6.35 g of copper ( Cu ).

Q. A current of $19296 C$ is passed through an aqueous solution of copper sulphate using copper electrodes. What is the mass (in $g$ ) of copper deposited at the cathode? (Molar mass of $C u = 63.5 g m o l^{- 1}$ )

3.17

1.58

6.35

0.79

Given,

Charge used $= 19296 C$

Molar mass of $C u = 63.5$

$∵ C u$ in $C u S O_{4}$ has $C u^{2 +}$ charge means:

$2 \times 96500 C$ of charge give $= 63.5 g$ of $C u$

Thus, $19296 C$ of charge give $= \frac{63.5 \times 19296}{2 \times 96500}$

$= 6.35 g$ of copper $(C u)$ .

Q. A current of 19296C is passed through an aqueous solution of copper sulphate using copper electrodes. What is the mass (in g ) of copper deposited at the cathode? (Molar mass of Cu=63.5gmol−1 )