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

Question

Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 mA current. The time required to liberate 0.01 mole of H2 gas at the cathode is (1 F = 96500 C mol-1) (A) 9.65 × 104 s (B) 19.3 × 104 s (C) 28.95 × 104 s (D) 38.6 × 104 s

Tardigrade Admin · Accepted Answer

0.01 mol of H2 = 0.02 g equivalent ⇒ Coulombs required = 0.02 × 96500=1930 C ⇒ Q=It= 1930 C ⇒ t= (1930/10 × 10-3)=19.3 × 104 s

Q. Electrolysis of dilute aqueous $N a Cl$ solution was carried out by passing $10 m A$ current. The time required to liberate $0.01$ mole of $H_{2}$ gas at the cathode is
$(1 F = 96500 C m o l^{- 1})$

$9.65 \times 1 0^{4} s$

$19.3 \times 1 0^{4} s$

$28.95 \times 1 0^{4} s$

$38.6 \times 1 0^{4} s$

$0.01 m o l$ of $H_{2} = 0.02 g$ equivalent
$\Rightarrow$ Coulombs required $= 0.02 \times 96500 = 1930 C$
$\Rightarrow Q = I t = 1930 C$
$\Rightarrow t = \frac{1930}{10 \times 1 0 ^{- 3}} = 19.3 \times 1 0^{4} s$

Q. Electrolysis of dilute aqueous NaCl solution was carried out by passing 10mA current. The time required to liberate 0.01 mole of H2​ gas at the cathode is (1F=96500Cmol−1)

9.65×104s

19.3×104s

28.95×104s

38.6×104s