JEE MAIN - Chemistry (2022 - 29th June Morning Shift - No. 13)
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
127
Explanation
$2 \mathrm{~F}$ produces $=\frac{3}{2}$ mole of gas
$0.10 \times 2 \times 3600$ coulomb produces
$$ \begin{aligned} & =\frac{\frac{3}{2} \times 0.1 \times 2 \times 3600}{2 \times 96500} \\\\ & =0.0056 \text { moles of gas } \end{aligned} $$
Volume of gas produced $=0.0056 \times 22.7 \mathrm{~L}$
$$ \begin{aligned} & \simeq 0.127 \mathrm{~L} \\\\ & =127 \mathrm{~mL} \end{aligned} $$
$0.10 \times 2 \times 3600$ coulomb produces
$$ \begin{aligned} & =\frac{\frac{3}{2} \times 0.1 \times 2 \times 3600}{2 \times 96500} \\\\ & =0.0056 \text { moles of gas } \end{aligned} $$
Volume of gas produced $=0.0056 \times 22.7 \mathrm{~L}$
$$ \begin{aligned} & \simeq 0.127 \mathrm{~L} \\\\ & =127 \mathrm{~mL} \end{aligned} $$
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