Consider the redox reaction- 2 S 2 O 32- I 2- S 4 O 62-2 I -A- I 2 gets oxidised to I -B- I 2 gets reduced to IC- S 2 O 32- gets reduced to S 4 O 62D- S 4 O 62- gets oxidised to S 2 O 32

The correct option is B I_2 gets reduced to nbsp; I^ nbsp;The given reaction is: 2S_2O^2 _3 + I_2 → S_4O^2 _6 + 2I^ Oxidation half reaction: +2S_2O^2 ...

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Standard XII

Chemistry

Redox Reactions

Consider the ...

Question

Consider the redox reaction: $2 S_{2} O_{3}^{2 -} + I_{2} \to S_{4} O_{6}^{2 -} + 2 I^{-}$

S_{4} O_{6}^{2 -} gets oxidised to S_{2} O_{3}^{2 -}

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S_{2} O_{3}^{2 -} gets reduced to S_{4} O_{6}^{2 -}

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I_{2} gets oxidised to I^{-}

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I_{2} gets reduced to I^{-}

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Solution

The correct option is D $I_{2} gets reduced to I^{-}$
The given reaction is:
$2 S_{2} O_{3}^{2 -} + I_{2} \to S_{4} O_{6}^{2 -} + 2 I^{-}$

Oxidation half-reaction: $+ 2 S_{2} O_{3}^{2 -} \to + 2.5 S_{4} O_{6}^{2 -}$
Here, $S_{2} O_{3}^{2 -}$ is getting oxidised to $S_{4} O_{6}^{2 -}$ as oxidation number of S is increasing from +2 to +2.5

Reduction half-reaction: ${0 I}_{2} \to - 1 2 I^{-}$
here $I_{2}$ is getting reduced to $2 I^{-}$ as oxidation number of S is decreasing from 0 to -1

So, (d) is the correct answer.

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Similar questions

Q. For the reaction

I_{2} + 2 S_{2} O_{3}^{2 -} \to S_{4} O_{6}^{2 -} + 2 I^{⊖}

\frac{- d [I_{2}]}{d t} = - \frac{1}{2} \frac{d [S_{2} O_{3}^{2 -}]}{d t}

II.

\frac{- d [I_{2}]}{d t} = - 2 \frac{d [S_{2} O_{3}^{2 -}]}{d t}

III.

\frac{- d [I_{2}]}{d t} = - 2 \frac{d [I^{⊖}]}{d t} \frac{d [S_{2} O_{3}^{2 -}]}{d t}

IV.

\frac{d [S_{4} O_{6}^{2 -}]}{d t} = \frac{1}{2} \frac{d [I^{⊖}]}{d t}

The correct option is:

Q. The order of increasing Oxidation number of

S

S_{8}, S_{2} O_{8}^{2 -}, S_{2} O_{3}^{2 -}, S_{4} O_{6}^{2 -}

is:

Q. What is redox reaction? In the reaction

Z n O + C \to Z n + C O

which substance gets oxidised and which gets reduced?

Which of the statements about the reaction below are incorrect?

(a) Lead is getting reduced.

(b) Carbon dioxide is getting oxidised.

(d) Lead oxide is getting reduced.

(i) (a) and (b)

(ii) (a) and (c)

(iii) (a), (b) and (c)

(iv) all

Q. Assertion :In the reaction,

2 S_{2} O_{3}^{2 -} + I_{2} \to S_{4} O_{6}^{2 -} + 2 I^{-}; I_{2}

is oxidised. Reason: During oxidation, loss of electron takes place.

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Redox Reactions

Standard XII Chemistry

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Consider the redox reaction: 2S2O2−3+I2→S4O2−6+2I−

Consider the redox reaction: $2 S_{2} O_{3}^{2 -} + I_{2} \to S_{4} O_{6}^{2 -} + 2 I^{-}$