The above reaction was studied at 300 K by monitoring the concentration of in which initial concentration was 10 M and after half an hour became 8.8 M. The rate of production of is ______ (Nearest Integer) [2023]

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Solution

Q.
${KClO}_{3} + 6 {FeSO}_{4} + 3 H_{2} {SO}_{4} \to KCl + 3 {Fe}_{2} {({SO}_{4})}_{3} + 3 H_{2} O$

The above reaction was studied at 300 K by monitoring the concentration of ${FeSO}_{4}$ in which initial concentration was 10 M and after half an hour became 8.8 M. The rate of production of ${Fe}_{2} {({SO}_{4})}_{3}$ is ______ $\times 10^{- 6}$ ${mol L}^{- 1} s^{- 1} .$ (Nearest Integer) [2023]

Ans.
(333)

${KClO}_{3} + 6 {FeSO}_{4} + 3 H_{2} {SO}_{4} \to KCl + 3 {Fe}_{2} {({SO}_{4})}_{3} + 3 H_{2} O$

$ROR = - \frac{Δ [{KClO}_{3}]}{Δ t} = \frac{- 1}{6} \frac{Δ [{FeSO}_{4}]}{Δ t}$

$= \frac{+ 1}{3} \frac{Δ [{Fe}_{2} {({SO}_{4})}_{3}]}{Δ t}$

$\frac{Δ [{Fe}_{2} {({SO}_{4})}_{3}]}{Δ t} = \frac{1}{2} \frac{- Δ [{FeSO}_{4}]}{Δ t}$

$= \frac{1}{2} \frac{(10 - 8.8)}{30 \times 60}$

$= 0.333 \times 10^{- 3}$

$= 333 \times 10^{- 6} {mol litre}^{- 1} {sec}^{- 1}$

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