How much time approximately would it take in minutes to deposit 1.18 g of metallic copper on a metal object when a current of 2.0 A is passed through the electrolytic cell containing Cu 2+ ions?

Question

How much time approximately would it take in minutes to deposit 1.18 g of metallic copper on a metal object when a current of 2.0 A is passed through the electrolytic cell containing Cu 2+ ions? (A) 10 min (B) 20 min (C) 30 min (D) 40 min

Tardigrade Admin · Accepted Answer

According to Faraday's first law: w=Z I t w=1.18 g , Z=(63.5/2 × 96500), I=2 A t=(w/Z I)=(1.18/63.5 × 2) × 2 × 96500=1793 s or (1793/60) ≈ 30 mins

Q. How much time approximately would it take in minutes to deposit $1.18 g$ of metallic copper on a metal object when a current of $2.0 A$ is passed through the electrolytic cell containing $C u^{2 +}$ ions?

$10 min$

$20 min$

$30 min$

$40 min$

According to Faraday's first law:

$w = Z I t$

$w = 1.18 g, Z = \frac{63.5}{2 \times 96500}, I = 2 A$

$t = \frac{w}{Z I} = \frac{1.18}{63.5 \times 2} \times 2 \times 96500 = 1793 s$ or $\frac{1793}{60} \approx 30 min s$

Q. How much time approximately would it take in minutes to deposit 1.18g of metallic copper on a metal object when a current of 2.0A is passed through the electrolytic cell containing Cu2+ ions?

10min

20min

30min

40min