Question

A steady current of 5 A is maintained for 45 minutes. During this time it deposits 4.572 g of zinc at the cathode of voltameter. Electrochemical equivalent of zinc is:

• A. $3.387\times {10}^{-4}g/C$
• B. $3.387\times {10}^{-4}kg/C$
• C. $3.384\times {10}^{-4}kg/C$
• D. $3.384\times {10}^{-3}kg/C$

Answer 1

Answer: (A)

$3.387\times {10}^{-4}g/C$

The electrochemical equivalent of a chemical element is the mass of that element (in grams) transported by 1 coulomb of electricity. The mass of a substance liberated or deposited at an electrode during electrolysis is directly proportional to the quantity of charge passed through the electrolyte.

$m=ZIt$

Electrochemical equivalent $Z=\frac{m}{It}=\frac{4.572}{5\times 45\times 60}=3.387\times {10}^{-4}g/C$