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Oxidation and Reduction

How H 2+ Cl 2...

Question

How $H_{2} + C l_{2} \to 2 H C l$ can be a redox reaction?

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Solution

Look at the oxidation state of reactants and products.
Hydrogen in the reactant side has oxidation state 0 similar to chlorine. In HCl, hydrogen has an oxidation state of +1, and Cl has an oxidation state of -1.
So, hydrogen moves from 0 to +1, clearly increase in oxidation state( oxidation) whereas chlorine goes from 0 to -1, a decrease in the oxidation state (reduction).
So, it is a clearly a redox reaction.

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Q. H2S + Cl2 ---> 2HCl + S

Prove that the given reaction is a redox reaction, stating reasons and define it.

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

Q. In the reaction

H_{2} S + C l_{2} \to 2 H C l + S

, the oxidizing agent is :

H_{2} + C l_{2} ⟶ 2 H C l

The above reaction is an example of which of the following reaction?

C l_{2} + H_{2} S \to 2 H C l + S

, In the reaction, oxidation state of chlorine changes from.

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