Chemistry-(general)
NEET Chemistry (general) MCQ Question
Type: MCQ-numerical-Hard-Class 12
Calculate the time in seconds for which a current of 1.5 amperes must flow to deposit 1.45 g of silver from AgNO3 solution. (Given: Molar mass of Ag = 107.87 g/mol, Faraday's constant = 96500 C/mol)
A
1250 s
B
1300 s
C
1200 s
D
1350 s
Correct Answer
Option A
Detailed Explanation
Using Faraday's laws, the amount of silver deposited is given by m = (Q/F) × (M/z), where Q = It, M = molar mass, z = valency. Solving for t: 1.45 = (1.5 * t / 96500) * (107.87 / 1), gives t = 1250 s.
Found an issue with this question?