KCET · Chemistry · Chemical Kinetics
By passing electric current, \( \mathrm{NaClO}_{3} \) is converted into \( \mathrm{NaClO}_{4} \) according to the following
equation
\( \mathrm{NaClO}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{NaClO}_{4}+\mathrm{H}_{2} \)
How many moles of \( \mathrm{NaClO}_{4} \) will be formed when three Faradays of charge is passed
through \( \mathrm{NaClO}_{3} \) ?
- A \( 0.75 \)
- B \( 1.0 \)
- C \( 1.5 \)
- D \( 3.0 \)
Answer & Solution
Correct Answer
(C) \( 1.5 \)
Step-by-step Solution
Detailed explanation
\(\mathrm{NaClO}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{NaClO}_{4}+\mathrm{H}_{2}\)
\(x=+5\)
Change in number of electrons \(=2\)
mole of \(\mathrm{NaClO}_{3}\) required \(2 \mathrm{~F}\) of charge to convert into 1 mole of \(\mathrm{NaClO}_{4}\)
\(\Rightarrow 1 \mathrm{~F}\) will convert \(^{1 / 2}\) moles of \(\mathrm{NaClO}_{3}\) into \(\mathrm{NaClO}_{4}\)
\(\Rightarrow 3 \mathrm{~F}=\frac{1}{2} \times 3\) moles of \(\mathrm{NaClO}_{4}\)
\(=1.5\) mol.
\(x=+5\)
Change in number of electrons \(=2\)
mole of \(\mathrm{NaClO}_{3}\) required \(2 \mathrm{~F}\) of charge to convert into 1 mole of \(\mathrm{NaClO}_{4}\)
\(\Rightarrow 1 \mathrm{~F}\) will convert \(^{1 / 2}\) moles of \(\mathrm{NaClO}_{3}\) into \(\mathrm{NaClO}_{4}\)
\(\Rightarrow 3 \mathrm{~F}=\frac{1}{2} \times 3\) moles of \(\mathrm{NaClO}_{4}\)
\(=1.5\) mol.
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