A dilute solution of sulphuric acid is electrolysed using a current of 0.10 A for 2 hours to produce hydrogen and oxygen gas. The total volume of gases produced a STP is _____________ cm3. (Nearest integer)
[Given : Faraday constant F = 96500 C mol$-$1 at STP, molar volume of an ideal gas is 22.7 L mol$-$1]
Answer (integer)
127
Solution
$2 \mathrm{~F}$ produces $=\frac{3}{2}$ mole of gas
<br/><br/>
$0.10 \times 2 \times 3600$ coulomb produces
<br/><br/>
$$
\begin{aligned}
& =\frac{\frac{3}{2} \times 0.1 \times 2 \times 3600}{2 \times 96500} \\\\
& =0.0056 \text { moles of gas }
\end{aligned}
$$<br/><br/>
Volume of gas produced $=0.0056 \times 22.7 \mathrm{~L}$
<br/><br/>
$$
\begin{aligned}
& \simeq 0.127 \mathrm{~L} \\\\
& =127 \mathrm{~mL}
\end{aligned}
$$
About this question
Subject: Chemistry · Chapter: Electrochemistry · Topic: Electrochemical Cells
This question is part of PrepWiser's free JEE Main question bank. 127 more solved questions on Electrochemistry are available — start with the harder ones if your accuracy is >70%.