Question

which of the following is Redox reaction

Answer 1

The correct answers are option (2) N₂O₅ + H₂O -----> Agl + KNO₃ and

(3) BaO₂ + H₂SO₄ -----> BaSO₄ + H₂O.

• Redox reaction is a chemical reaction that reduces oxidation when reactants make changes in their oxidation conditions. The term 'redox' is a short form of oxidation. All redox reactions can be divided into two distinct processes - the reduction process and the oxidation process.
• A substance that is reduced in chemical reactions is known as an oxidizing agent, while a substance that is oxidized is known as a reducing agent.

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Answer 2

Answer:

4. $SnCl_2+HgCl_2 \rightarrow SnCl_4 + Hg$ is the redox reactions among the given options.

Explanation:

• A redox reaction, as the name says, is a reduction-oxidation reaction, i.e., one reactant gets reduced (oxidant), while the other, is oxidized (reductant).

Here,

1. $N_2O_5 + H_2O \rightarrow 2HNO_3$
   Here, N is in the +5 oxidation state on both sides of the reaction, i.e., its oxidation state is unchanged.
   Thus, no, it isn't a redox reaction.
2. $AgNO_3+KI\rightarrow AgI+KNO_3$
   Here, Ag and K are in the +1 oxidation state on both sides of the reaction, implying that no reduction/oxidation takes place.
   Thus, it isn't a redox reaction.
3. $BaO_2+H_2SO_4 \rightarrow BaSO_4 +H_2O_2$
   Here, Ba remains in the +2 oxidation state throughout the reaction, thereby proving that neither reduction nor oxidation is taking place.
   Thus, it isn't a redox reaction.
4. $SnCl_2+HgCl_2 \rightarrow SnCl_4 + Hg$
   Here, on the reactants' side, Sn and Hg are in the +2 state.
   However, on the products' side, Sn is in its +4 state, while Hg is in its 0 state, implying that Sn has been oxidized, while Hg has been reduced.
   We can also call Hg the oxidant and Sn the reductant.
   
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