How much current is required to produce \(\mathrm{H}_2\) gas at the rate of \(1 \mathrm{cc} / \mathrm{sec}\)…
How much current is required to produce \(\mathrm{H}_2\) gas at the rate of \(1 \mathrm{cc} / \mathrm{sec}\) under STP?
- \(2.33 \mathrm{~A}\)
- \(6.0 \mathrm{~A}\)
- \(7.9 \mathrm{~A}\)
- \(8.61 \mathrm{~A}\)
Solution
\(2 \mathrm{H}^{+}+2 e^{-} \longrightarrow \mathrm{H}_2\)
1 mole of \(\mathrm{H}_2=22400 \mathrm{cc}\) at NTP
2 moles of electron required \(=2 \times 96500\)
\(\therefore 1 \mathrm{cc}\) at \(\mathrm{NTP}=\frac{2 \times 96500}{22400}=8.616\)
\(\begin{array}{ll}
\therefore & Q=I t \\
\Rightarrow & I=\frac{8.616}{l}=8.616 Å
\end{array}\)
Hence, option (d) is correct.
Asked in: AP EAMCET 2020 (21 Sep Shift 2)
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