Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milli ampere current. The time required to liberate 0.01 mol of H2 gas at the cathode is (1 Faraday = 96500 C mol-1)a)9.65 x 104secb)19.3 x 104secc)28.95 x 104secd)38.6 x 104secCorrect answer is option 'B'. Can you explain this answer?

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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 mol of H₂ gas at the cathode is (1 Faraday = 96500 C mol^-1)

a)
9.65 x 10⁴ sec
b)
19.3 x 10⁴ sec
c)
28.95 x 10⁴ sec
d)
38.6 x 10⁴ sec

Correct answer is option 'B'. Can you explain this answer?

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Electrolysis of dilute aqueous NaCl solution was carried out by passin...

According to Faraday's first law of electrolysis:
m = EIt/F
Where:
m = mass of substance
E = equivalent weight of substance
I = current in amperes
t = time required
F = 96,500 Coulombs

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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 mol of H2 gas at the cathode is (1 Faraday = 96500 C mol-1)

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Chemical reactions involve interaction of atoms and molecules. A large number of atoms/molecules (approximately 6.023 × 1023) are present in a few grams of any chemical compound varying with their atomic/molecular masses. To handle such large numbers conveniently, the mole concept was introduced.This concept has implications in diverse areas such as analytical chemistry, biochemistry, electrochemistry and radiochemistry. The following example illustrates a typical case, involving chemical/electrochemical reaction, which requires a clear understanding of the mole concept. A 4.0 molar aqueous solution NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass: Na = 23, Hg = 200; 1 Faraday = 96,500 coulombs)If the cathode is a Hg electrode, the maximum weight (g) of amalgam formed from this solution is Correct answer is '446'. Can you explain this answer?

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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 mol of H2 gas at the cathode is (1 Faraday = 96500 C mol-1)a)9.65 x 104secb)19.3 x 104secc)28.95 x 104secd)38.6 x 104secCorrect answer is option 'B'. Can you explain this answer?

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