Question

The number of moles of electrons passed when a current of $2A$ is passed through a solution of electrolyte for $20$ minutes is:

• (A) $4.1\times {10}^{-4}$ mole
• (B) $1.24\times {10}^{-2}$ mole
• (C) $2.487\times {10}^{-2}$ mole
• (D) $2.487\times {10}^{-1}$ mole

Hint:

Calculation of Number of Moles of Electrons
Given:

• Current \( I = 2 \) A (Amperes)
• Time \( t = 20 \) minutes = \( 20 \times 60 \) seconds = \( 1200 \) seconds
• Total charge \( Q = I \cdot t = 2 \, \text{A} \times 1200 \, \text{s} = 2400 \) C (Coulombs)
• Faraday's constant \( F = 96500 \, \text{C/mol} \)

Calculation:

• Number of moles of electrons \( n = \frac{Q}{F} = \frac{2400 \, \text{C}}{96500 \, \text{C/mol}} = 2.487 \times 10^{-2} \) moles

Conclusion:
Therefore, option C is correct.

Answer 1

The Correct Option is C

Explanation:
Current passed, $I=2A$Time for which current is passed $t=20min=20min\times 60s/min=1200s$So, total charge flown, $Q=It=2A\times 1200s=2400C$Number of moles of electrons $n=\frac{Q}{96500}=\frac{2400C}{96500C/mol{e}^{-}}=2.487\times {10}^{-2}$ molesHence, the correct option is (C).