${KClO}_{3} + 6 {FeSO}_{4} + 3 H_{2} {SO}_{4} \to KCl + 3 {Fe}_{2} {({SO}_{4})}_{3} + 3 H_{2} O$
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 ________ $\times 10^{- 6} mol L^{- 1} s^{- 1}$ .

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answer is 333.

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Detailed Solution

Rate of disappearance of ${Fe}_{2} {({SO}_{4})}_{3} = \frac{1}{2}$ (Rate of disappearance of ${FeSO}_{4}$ )
$= \frac{1}{2} (\frac{1.2}{1800}) m . \sec^{- 1}$
$= 333.3 \times 10^{- 6} M . \sec^{- 1}$
$= 333 \times 10^{- 6} M . \sec^{- 1}$ (nearest integer)