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Types of Redox Reactions

In the follow...

Question

In the following reaction : $C r (O H)_{3} + O H^{-} + I O_{3}^{-} \to C r O_{4}^{2 -} + H_{2} O + I^{-}$ :

A

I O_{3}^{-}

is oxidising agent

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B

C r (O H)_{3}

is oxidised

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C

6 e^{-}

are being taken per iodine atom

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D

all of these

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Solution

The correct option is D all of these
Balanced chemical equation is,
$2 C r (O H)_{3} + I O_{3}^{-} + 4 O H^{-} \to 2 C r O_{4}^{2 -} + I^{-} + 5 H_{2} O$
$I^{5 +} + 6 e^{-} \to I^{-}$ (Reduction)
Oxidation state of Cr is changing from +3 to +6,
$2 C r^{3 +} \to 2 C r^{6 +} + 6 e^{-}$ (Oxidation)
Hence $C r (O H)_{3}$ is oxidized and this implies $I O_{3}^{-}$ is oxidizing agent.

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Similar questions

Q. In the following reaction:

C r (O H)_{3} + (O H)^{-} + {I O_{3}}^{-} \to {C r O_{4}}^{2 -} + H_{2} O + I^{-}

Q. In the following reaction,

C r (O H)_{3} + O H^{-} + I O_{3}^{-} \to C r O_{4}^{2 -} + H_{2} O + I^{-}

Choose the incorrect statement:

Q. Balance the following equation by ion electron method:

C r (O H)_{3} + C l O^{-} + O H^{-} \to C r O_{4}^{2 -} + C l^{-} + H_{2} O

Q. The coefficients of

I^{-}

{I O_{3}}^{-}

H^{+}

in the following reactions in the balanced form respectively are:

I^{-} + {I O_{3}}^{-} + H^{+} \to I_{2} + H_{2} O

A) $N a_{2} O_{2} + H_{2} S O_{4} \to N a_{2} S O_{4} + H_{2} O_{2}$	1) Redox reaction
B) $H_{2} + C l_{2} \to 2 H C l$	2) Oxidation reaction
C) $C r (O H)_{3} \to C r O_{4}^{- 2}$	3) Non - redox reaction
D) $I O_{3}^{-} \to I^{-}$	4) Reduction reaction

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