1. Tardigrade
  2. Question
  3. Chemistry
  4. 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 Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

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 $Cu ^{2+}$ ions?

Electrochemistry

Solution:

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 $\frac{1793}{60} \approx 30 \,mins$