$\ce{KClO3 + 6 FeSO4 + 3 H2SO4 -> KCl + 3 Fe2(SO4)3 + 3 H2O}$ The above reaction was studied at 300 K by monitoring the concentration of $\ce{FeSO4}$ in which initial concentration was 10 M and after half an hour became 8.8 M. The rate of production of $\ce{Fe2(SO4)3}$ is $\_\_\_\_$ $\times 10^{-6} \mathrm{~mol~L^{-1}~s^{-1}}$. (Nearest integer)

JEE Main · 2023 · 11 Apr 2023 · Shift 1 · Chemical Kinetics

KClO X_{3} + 6 FeSO X_{4} + 3 H X_{2} SO X_{4} KCl + 3 Fe X_{2} (SO X_{4}) X_{3} + 3 H X_{2} O

The above reaction was studied at 300 K by monitoring the concentration of

FeSO X_{4}

in which initial concentration was 10 M and after half an hour became 8.8 M. The rate of production of

Fe X_{2} (SO X_{4}) X_{3}

____

\times 1 0^{- 6} mol L^{- 1} s^{- 1}

.
(Nearest integer)

Answer: 333

The rate of reaction connects each species through its stoichiometric coefficient:

- \frac{1}{6} \frac{Δ [ FeSO X _{4} ]}{Δ t} = \frac{1}{3} \frac{Δ [ Fe X _{2} ( SO X _{4} ) X _{3} ]}{Δ t}

, so the rate of formation of

Fe X_{2} (SO X_{4}) X_{3}

is one-half the rate of consumption of

FeSO X_{4}

. The iron(II) concentration falls by

10 - 8.8 = 1.2

M in 30 minutes

(1800 s)

, a consumption rate of

1.2/1800 = 6.67 \times 1 0^{- 4} mol L^{- 1} s^{- 1}

. Half of this is

3.33 \times 1 0^{- 4} mol L^{- 1} s^{- 1}

, so the rate of production of

Fe X_{2} (SO X_{4}) X_{3}

is 333

\times 1 0^{- 6} mol L^{- 1} s^{- 1}

JEE Main · 2023 · 11 Apr 2023 · Shift 1 · Integer answer