Q25 / 180 · KCET 2017 · Chemistry
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 \( \mathrm{NaClO}_{3} \) ?
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\( 1.0 \)
- Correct answerC\( 1.5 \)
- D\( 3.0 \)
Solution
$\mathrm{NaClO}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{NaClO}_{4}+\mathrm{H}_{2}$
$x=+5$
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.
Hence, the correct answer is option: 'C'.