NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

1 Hard

1 of 1

Application +4 | -1

Electrolysis of dilute aqueous NaCl solution was carried out by passing 10mA current. The time required to liberate 0.01 mole of

{\mathrm{H}_2}

gas at the cathode is (

1\mathrm{F} = 96500{\kern 1pt}{\kern 1pt}{\rm{C{\kern 1pt}{\kern 1pt}mo}}{\mathrm{l}^{ - 1}}

)

View answer and explanation

Correct option: B

19.3 \times {10^4}s

Option B (

19.3 \times {10^4}s

) is correct because the time required is calculated using Faraday's laws, relating current, moles of hydrogen, and Faraday's constant.

More Questions from ELECTRO CHEMISTRY

Practice All Chapter MCQs →

A{l^{3 + }}

{H_2}

{H^ + }

\mathrm{LiCl},{\rm{NaCl {\kern 1pt}{\kern 1pt}and {\kern 1pt}{\kern 1pt}KCl}}

\left(\mathrm{CuSO}_4\right)

\mathrm{A}{\mathrm{l}^{3 + }}