(A) $HOCl + H _{2} O _{2} \rightarrow H _{3} O ^{+}+ Cl ^{-}+ O _{2}$ (B) $I _{2}+ H _{2} O _{2}+2 OH ^{-} \rightarrow 2 I ^{-}+2 H _{2} O + O _{2}$ Choose the correct option.
$H _{2} O _{2}$ acts as reducing and oxidising agent respectively in equation (A) and (B)
$H _{2} O _{2}$ acts as oxidising agent in equation (A) and $( B )$
$H _{2} O _{2}$ acts as reducing agent in equation (A) and $( B )$
$H _{2} O _{2}$ act as oxidizing and reducing agent respectively in equation (A) and (B)
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The Correct Option isC
Solution and Explanation
The given problem involves two chemical reactions, and we need to identify the role of hydrogen peroxide, $H_2O_2$, in each of them. The reactions are:
Let's analyze the role of $H_2O_2$ in each equation:
Reaction A Analysis:
Reduction/Oxidation of $H_2O_2$:
$H_2O_2$ produces $O_2$. The transition from -1 oxidation state in $H_2O_2$ to zero in $O_2$ indicates oxidation. Since $H_2O_2$ loses electrons, it acts as a reducing agent.
Reaction B Analysis:
Reduction/Oxidation of $H_2O_2$:
$H_2O_2$ again produces $O_2$. Following the same logic of oxidation state change from -1 to zero, $H_2O_2$ is oxidized and acts as a reducing agent in this reaction as well.
Conclusion: In both reactions, $H_2O_2$ undergoes oxidation and therefore acts as a reducing agent in equations (A) and (B).
Therefore, the correct choice is:
$H_2O_2$ acts as a reducing agent in equation (A) and (B).
Redox reactions are chemical reactions where oxidation and reduction take place simultaneously. In this type of reaction, there is a gain of electrons for one chemical species while the other loses electrons or simply involves transfer of electrons. The species that loses electrons is oxidized while the one that gains electrons is reduced.
Types of Redox Reactions:
Redox reactions can be differentiated into 4 categories namely combination reactions, decomposition reactions, displacement reactions, and disproportionation reactions. Each is explained separately below:
Combination Reaction:
In this, the molecules combine to form new compounds. For example, when magnesium reacts to nitrogen.
Decomposition Reaction:
Opposite to the combination reaction, here there is a breakdown of compounds to simpler substances. For example, electrolysis of water.
Displacement Reaction:
In this, the more reactive metal will displace the less reactive one in a chemical reaction. The reactivity of an element is represented in a series called the reactivity series (arranged in decreasing order of reactivity) which makes it easier to determine the chemical reaction and its products.
Disproportionation Reaction:
This is a peculiar type of reaction where an element showing a particular oxidation state will be oxidized and reduced simultaneously. Another thing to note is that these reactions will always have an element that can exhibit three oxidation states.
