Consider the following redox reaction -2 S 2 O 32- I 2- S 4 O 62-2 I -Choose the correct statements-A- S 2 O 32- gets oxidised to S 4 O 62-B- S 2 O 32- gets reduced to S 4 O 62-C-I 2 gets reduced to I -D- I 2 gets oxidised to I

The correct options are A S_2O^2 _3 gets oxidised to nbsp; S_4O^2 _6 nbsp; C I_2 gets reduced to nbsp; I^ nbsp;The given reaction is: 2S_2O^2 _3 + ...

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Standard XII

Chemistry

Valency and Oxidation State

Consider the ...

Question

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

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

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

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Solution

The correct options are
A $S_{2} O_{3}^{2 -} gets oxidised to S_{4} O_{6}^{2 -}$
C
$I_{2} gets reduced to I^{-}$
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 :
${0 I}_{2} \to^{-}$
Here $I_{2}$ is getting reduced to $I^{-}$ since oxidation number of iodine changes from $0$ to $- 1$

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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. 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.

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. For the following oxidation half reaction,

2 S_{2} O_{3}^{2 -} (Reducing ~agent) \to S_{4} O_{6}^{2 -} + 2 e^{-}

Calculate the equivalent weight of

S_{2} O_{3}^{2 -}

.
(Given:

M

is the molecular weight of

S_{2} O_{3}^{2 -}

)

Q. For the following oxidation half reaction,

2 S_{2} O_{3}^{2 -} (Reducing ~agent) \to S_{4} O_{6}^{2 -} + 2 e^{-}

Calculate the equivalent weight of

S_{2} O_{3}^{2 -}

.
(Given:

M

is the molecular weight of

S_{2} O_{3}^{2 -}

)

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Valency and Oxidation State

Standard XII Chemistry

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Consider the following redox reaction : 2S2O2−3+I2→S4O2−6+2I− Choose the correct statements:

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