KCET · Chemistry · Electrochemistry
In the electrolysis of acidulated water, it is desired to obtain \(1.12\) cc of hydrogen per second under STP condition. The current to be passed is
- A \(1.93 \mathrm{~A}\)
- B \(9.65 \mathrm{~A}\)
- C \(19.3 \mathrm{~A}\)
- D \(0.965 \mathrm{~A}\)
Answer & Solution
Correct Answer
(B) \(9.65 \mathrm{~A}\)
Step-by-step Solution
Detailed explanation
No. of moles of \(\mathrm{H}_{2}=\frac{1.12}{22400}\)
No. of equivalence of hydrogen
\[
=\frac{1.12 \times 2}{22400}=10^{-4}
\]
No. of Faradays required \(=10^{-4}\)
\(\therefore\) Current to be passed in one second
\[
\begin{aligned}
&=96500 \times 10^{-4} \\
&=9.65 \mathrm{~A}
\end{aligned}
\]
No. of equivalence of hydrogen
\[
=\frac{1.12 \times 2}{22400}=10^{-4}
\]
No. of Faradays required \(=10^{-4}\)
\(\therefore\) Current to be passed in one second
\[
\begin{aligned}
&=96500 \times 10^{-4} \\
&=9.65 \mathrm{~A}
\end{aligned}
\]
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