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Chemical Properties

In the follow...

Question

In the following reaction which substance is oxidised and which one is reduced?
$I_{2} + N a O H \to N a I O_{3} + N a I + H_{2} O$

A

I_{2}, N a O H

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B

N a O H, I_{2}

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C

I_{2}, I_{2}

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D

N a O H, N a O H

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Solution

The correct option is C $I_{2}, I_{2}$
$0 3 I_{2} + 6 N a O H \to N a + 5 I O_{3} + 5 N a - 1 I + 3 H_{2} O$

We can clearly see that $I_{2}$ is itself oxidised as well as reduced (disproportionation).

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Q. In the following reaction which substance is oxidised and which one is reduced?

I_{2} + N a O H \to N a I O_{3} + N a I + H_{2} O

Q. In the following Reaction, which substance is oxidised and reduced?

I_{2} + N a O H \to I O_{3} + N a I + 3 H_{2} O

Q. In the following reactions:

A l C l_{3} + 3 K \to A l + 3 K C l

S O_{2} + 2 H_{2} S \to 3 S + H_{2} O

3 I_{2} + 6 N a O H \to N a I O_{3} + 5 N a I + 3 H_{2} O

Identify the correct option which represents the oxidised substances?

Q. Balance the following equation by oxidation number method.

I_{2} + N a O H \to N a I O_{3} + N a I + H_{2} O

Q. Which substance/ion is oxidised and which substance/ion is reduced in the following reaction?

C l_{2} + S O_{3}^{2 -} + H_{2} O \to 2 C l^{-} + S O_{4}^{2 -} + 2 H^{+}

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