How many electrons would be required to deposit 6.35 g of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate ? (Atomic mass of copper = 63.5 u, NA = Avogadro's constant) :

Question

How many electrons would be required to deposit 6.35 g of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate ? (Atomic mass of copper = 63.5 u, NA = Avogadro's constant) : (A) (NA/20) (B) (NA/10) (C) (NA/5) (D) (NA/2)

Tardigrade Admin · Accepted Answer

W =( E /96500) × Q ⇒ 6.35 =(63.5/2 × 96500) × Q ⇒ Q =2 × 9650 coulomb ⇒ 1 F = charge of 1 mol of e -=96500 ∴ No. of e - =( N A /10) × 2 =( N A /5)

Q. How many electrons would be required to deposit $6.35 g$ of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate ? (Atomic mass of copper $= 63.5 u, N_{A} =$ Avogadro's constant) :

$\frac{N _{A}}{20}$

$\frac{N _{A}}{10}$

$\frac{N _{A}}{5}$

$\frac{N _{A}}{2}$

$W = \frac{E}{96500} \times Q$

$\Rightarrow 6.35 = \frac{63.5}{2 \times 96500} \times Q$

$\Rightarrow Q = 2 \times 9650$ coulomb

$\Rightarrow 1 F =$ charge of $1$ mol of $e^{-} = 96500$

$∴$ No. of $e^{-} = \frac{N _{A}}{10} \times 2$

$= \frac{N _{A}}{5}$

Q. How many electrons would be required to deposit 6.35g of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate ? (Atomic mass of copper =63.5u,NA​= Avogadro's constant) :

20NA​​

10NA​​

5NA​​

2NA​​