An electrolytic cell is composed of Cu and Zn. A current of 9.65 A is drawn from a cell for 1 hour. Then the loss in mass at anode and gain in mass at cathode, respectively could be

Question

An electrolytic cell is composed of Cu and Zn. A current of 9.65 A is drawn from a cell for 1 hour. Then the loss in mass at anode and gain in mass at cathode, respectively could be (A) 11.77 g, 11.43 g (B) 11.77 g, 10 g (C) 22.86 g, 23.54 g (D) 23.54 g, 22.86 g

Tardigrade Admin · Accepted Answer

For Cu (at cathode) W =( E /96500) × it =((63.5/2)/96500) × 9.65 × 1 × 60 × 60=11.43 g E=( text molar mass /n- text factor )=(63.5/2 arrow(C u+2))

Q. An electrolytic cell is composed of $C u$ and $Z n$ . A current of $9.65 A$ is drawn from a cell for $1$ hour. Then the loss in mass at anode and gain in mass at cathode, respectively could be

11.77 g, 11.43 g

11.77 g, 10 g

22.86 g, 23.54 g

23.54 g, 22.86 g

For $C u$ (at cathode)
$W = \frac{E}{96500} \times i t = \frac{\frac{63.5}{2}}{96500} \times 9.65 \times 1 \times 60 \times 60 = 11.43 g$
$E = \frac{molar mass}{n - factor} = \frac{63.5}{2 \leftarrow ( C u ^{+ 2} )}$

Q. An electrolytic cell is composed of Cu and Zn. A current of 9.65A is drawn from a cell for 1 hour. Then the loss in mass at anode and gain in mass at cathode, respectively could be