The reduction of peroxydisulphate ion by I- ion is expressed by S2O82-3I- - 2SO42-I3-If the rate of disappearance of I- is 9-2 - 10-3 mol-L-1 s-1- what is the rate of formation of SO42- during the same time-

Reduction reaction of peroxydisulphateion: S_2O_8^2 +3I^ → 2SO_4^2 +I_3^ ∴ d[S_2O_8]^2 dt= 13d[I^ ]dt=12d[SO_4^2 ]dt=d[I_3^ ]dt So; 13d[I^ ]dt=12d[SO_4^2 ...

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Byju's Answer

Standard XII

Chemistry

Types of Elementary Reactions

The reduction...

Question

The reduction of peroxydisulphate ion by $I^{-}$ ion is expressed by $S_{2} O_{8}^{2 -} + 3 I^{-} \to 2 S O_{4}^{2 -} + I_{3}^{-}$
If the rate of disappearance of $I^{-}$ is $9 / 2 \times 10^{- 3} {mol/L}^{- 1} s^{- 1}$ , what is the rate of formation of $S O_{4}^{2 -}$ during the same time?

10^{- 3} {mol/L}^{- 1} s^{- 1}

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2 \times 10^{- 3} {mol L}^{- 1} s^{- 1}

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3 \times 10^{- 3} {mol L}^{- 1} s^{- 1}

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4 \times 10^{- 3} {mol L}^{- 1} s^{- 1}

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Solution

The correct option is C $3 \times 10^{- 3} {mol L}^{- 1} s^{- 1}$
Reduction reaction of peroxydisulphateion:
$S_{2} O_{8}^{2 -} + 3 I^{-} \to 2 S O_{4}^{2 -} + I_{3}^{-}$
$∴ - \frac{d [S_{2} O_{8}]^{2 -}}{d t} = - \frac{1}{3} \frac{d [I^{-}]}{d t} = \frac{1}{2} \frac{d [S O_{4}^{2 -}]}{d t} = \frac{d [I_{3}^{-}]}{d t}$
So; $- \frac{1}{3} \frac{d [I^{-}]}{d t} = \frac{1}{2} \frac{d [S O_{4}^{2 -}]}{d t}$
$\frac{1}{3} \times \frac{9}{2} \times 10^{- 3} = \frac{1}{2} \frac{d [S O_{4}^{2 -}]}{d t}$
$\frac{d [S O_{4}^{2 -}]}{d t} = 3 \times 10^{- 3} {mol L}^{- 1} s^{- 1}$
Therefore the rate of appearance of $S O_{4}^{2 -}$ is $3 \times 10^{- 3} {mol L}^{- 1} s^{- 1}$

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Similar questions

Q. The oxidation of iodide ion by perdisulphate ion is described as follows :

I^{⊝} + S_{2} O_{8}^{2 -} \to I_{3}^{⊝} + S O_{4}^{2 -}

If the rate disappearance of

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Q. Consider the reaction:

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Q. The reaction

2 I^{-} (a q) + S_{2} O_{8}^{2 -} (a q) \to I_{2} (a q) + 2 S O_{4}^{2 -} (a q)

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25^{0} C

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where, Rate

= - \frac{d [S_{2} O_{8}^{2 -}]}{d t}

[I $^{-}$ ]	$[S_{2} O_{8}^{2 -}]$	Inital rate (mol L $^{- 1}$ S $^{- 1}$
0.08	0.040	$12.5 \times 10^{- 6}$
0.04	0.040	$6.25 \times 10^{- 6}$
0.08	0.020	$5.56 \times 10^{- 6}$
0.032	0.040	$4.35 \times 10^{- 6}$
0.060	0.030	$6.41 \times 10^{- 6}$

The value of the rate constant is:

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2 S O_{2} (g) + O_{2} (g) \to 2 S O_{3} (g)

The rate of
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L^{- 1} s e c^{- 1}

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The reduction of peroxydisulphate ion by I– ion is expressed by S2O2−8+3I−→2SO2−4+I−3 If the rate of disappearance of I– is 9/2×10–3 mol/L−1 s−1, what is the rate of formation of SO2−4 during the same time?

The reduction of peroxydisulphate ion by $I^{-}$ ion is expressed by $S_{2} O_{8}^{2 -} + 3 I^{-} \to 2 S O_{4}^{2 -} + I_{3}^{-}$
If the rate of disappearance of $I^{-}$ is $9 / 2 \times 10^{- 3} {mol/L}^{- 1} s^{- 1}$ , what is the rate of formation of $S O_{4}^{2 -}$ during the same time?