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Q.

Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milli ampere current. The time required to liberate 0.01 moles of H₂ gas at the cathode is (1 Faraday = 96500 C mol^-1)

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a

38.6 × 10⁴ sec

b

9.65 × 10⁴ sec

c

28.95 × 10⁴ sec

d

19.3 × 10⁴ sec

answer is B.

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Detailed Solution

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When dilute aqueous solution is electrolysed, at cathode, Hydrogen gas and at anode, Oxygen gas are liberated.
$2 H_{2} O + 2 e^{-} \to H_{2} .$
For liberation of 1 mole of H₂, 2 moles of e^- are required .
0.01 moles of H₂ will require 2 X 0.01 = 0.02 moles of electrons or 0.02 faradays.
Charge required = i X t
$Time (t) = \frac{Charge}{Current}$
i= 10 mill ampere = 10 X 10^-3 ampere.
$t = \frac{0.02 X 96500}{10 X 10^{- 3}} = 19.3 X 10^{4} seconds .$

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Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milli ampere current. The time required to liberate 0.01 moles of H2 gas at the cathode is (1 Faraday = 96500 C mol-1)