The Question is from neet-chemistry p-block-elements h2o2, and it was created by the author Mr. S M HUSSAIN

Question

A mixture of $H_2O_2$ and $KI$ liberates iodine. In this reaction, $H_2O_2$ acts as:

Mr. S M HUSSAIN · Accepted Answer

## CORE INFORMATION
✓ **Answer**: A
## CONCEPT FRAMEWORK
 **Primary Concept**: Redox reactions and identification of oxidizing and reducing agents
 **Related Topics**: Hydrogen peroxide reactions, iodine liberation
 **Prerequisites**: Understanding of oxidation states, oxidation and reduction processes
## SOLUTION PATHWAY
**Given Information**:
  The reaction between $H_2O_2$ and $KI$ produces iodine ($I_2$).
  We need to determine the role of $H_2O_2$ in this reaction.
**Method & Steps**:
 1. Write the balanced chemical equation for the reaction between $H_2O_2$ and $KI$.
  The reaction is:
  $H_2O_2 + 2KI + 2H^+ ightarrow I_2 + 2H_2O + 2K^+$
 2. Analyze the oxidation states of the elements involved.
  In $H_2O_2$, the oxidation state of oxygen is -1.  In $I_2$, the oxidation state of iodine is 0. In $KI$, the oxidation state of iodine is -1.
 3. Determine whether $H_2O_2$ is oxidized or reduced.
  The oxidation state of oxygen in $H_2O_2$ decreases from -1 to -2 in $H_2O$. This is a reduction.
  The oxidation state of iodine in $KI$ increases from -1 to 0 in $I_2$. This is an oxidation.
  Since $H_2O_2$ causes the oxidation of $I^-$, $H_2O_2$ acts as an oxidizing agent.
 4.  Confirm the role of $H_2O_2$.
  $H_2O_2$ is reduced, meaning it gains electrons.  A substance that gains electrons is an oxidizing agent (it oxidizes another substance).
  Result: $H_2O_2$ acts as an oxidizing agent.
  Verification: The balanced equation shows $H_2O_2$ is reduced while $KI$ is oxidized, confirming its role as an oxidizing agent.
 ## OPTION ANALYSIS
A ✓:  $H_2O_2$ is reduced in the reaction, meaning it accepts electrons from iodide ions ($I^-$), thus oxidizing them to iodine ($I_2$).  This is the definition of an oxidizing agent.
B :x: $H_2O_2$ is not a reducing agent in this reaction because it gains electrons itself.
C :x: $H_2O_2$ is a reactant, not a catalyst. A catalyst is not consumed in the reaction.
D :x: While $H_2O_2$ can be acidic, its primary role in this specific reaction is as an oxidizing agent.
 ## LEARNING AIDS
 **Common Mistakes**:
  1.Confusing oxidizing and reducing agents: Remember OIL RIG (Oxidation Is Loss, Reduction Is Gain) of electrons.  An oxidizing agent gains electrons and is reduced; a reducing agent loses electrons and is oxidized.
  2.Ignoring the balanced chemical equation: The balanced equation provides crucial information about changes in oxidation states and thus the role of each reactant.
 **Quick Tips**:
  1.Always determine the oxidation states of elements before deciding on whether a substance acts as an oxidizing or reducing agent.
  2.Remember that an oxidizing agent is reduced and a reducing agent is oxidized.

Mr. S M HUSSAIN · Answer

The correct Option is "An oxidizing agent"

Mr. S M HUSSAIN · Answer

A reducing agent

Mr. S M HUSSAIN · Answer

A catalyst

Mr. S M HUSSAIN · Answer

An acid

NEET Chemistry Hydrogen H2O2 MCQs

Select Topic

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

Question Tags

NEET Subjects

Our Bots

Company