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Hydrogen peroxide in its reaction with KIO4 and NH2OH respectively, is acting as a
- a)Reducing agent, oxidising agent
- b)Reducing agent, reducing agent
- c)Oxidising agent, oxidising agent
- d)Oxidising agent, reducing agent
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
Hydrogen peroxide in its reaction with KIO4 and NH2OH respectively, is...
Explanation:
Oxidizing Agent is defined as the agent which helps the other substance to get oxidized and itself gets reduced. The oxidation state of the oxidizing agent gets reduced.
Reducing Agent is defined as the agent which helps the other substance to get reduced and itself gets oxidized. The oxidation state of the reducing agent is increased.
1. Reaction of Hydrogen Peroxide with KIO4 follows the equation:
Oxidation state of Iodine on reactant side = +7
Oxidation state of Iodine on product side = +5
As, the oxidation state of iodine is getting reduced, hence it is getting reduced. So, it will act as oxidizing agent and h2O2 will act as reducing agent.
2. Reaction of Hydrogen Peroxide with NH2O4 follows the equation:
Oxidation state of Nitrogen on reactant side = -1
Oxidation state of Nitrogen on product side = +3
As, the oxidation state of nitrogen is increasing, hence it is getting oxidized. So, it will act as reducing agent and will act as oxidizing agent.
So, the correct option is option a.
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Oxidizing Agent is defined as the agent which helps the other substance to get oxidized and itself gets reduced. The oxidation state of the oxidizing agent gets reduced.
Reducing Agent is defined as the agent which helps the other substance to get reduced and itself gets oxidized. The oxidation state of the reducing agent is increased.
1. Reaction of Hydrogen Peroxide with KIO4 follows the equation:
Oxidation state of Iodine on reactant side = +7
Oxidation state of Iodine on product side = +5
As, the oxidation state of iodine is getting reduced, hence it is getting reduced. So, it will act as oxidizing agent and h2O2 will act as reducing agent.
2. Reaction of Hydrogen Peroxide with NH2O4 follows the equation:
Oxidation state of Nitrogen on reactant side = -1
Oxidation state of Nitrogen on product side = +3
As, the oxidation state of nitrogen is increasing, hence it is getting oxidized. So, it will act as reducing agent and will act as oxidizing agent.
So, the correct option is option a.
Most Upvoted Answer
Hydrogen peroxide in its reaction with KIO4 and NH2OH respectively, is...
Hydrogen peroxide (H2O2) can act as a reducing agent or an oxidizing agent depending on the reaction conditions and the other substances involved. In the reactions with KIO4 and NH2OH, it acts as a reducing agent.
I. Reaction with KIO4:
Hydrogen peroxide reacts with potassium iodate (KIO4) in an acidic medium to form iodine (I2) and oxygen gas (O2). The balanced equation for this reaction is:
2 H2O2 + 2 H+ + KIO4 → I2 + K+ + 4 H2O + O2
In this reaction, hydrogen peroxide is oxidized from the -1 oxidation state to the 0 oxidation state, while KIO4 is reduced from the +7 oxidation state to the +5 oxidation state. The hydrogen peroxide donates electrons to the iodate ion, causing its reduction.
II. Reaction with NH2OH:
Hydrogen peroxide also reacts with hydroxylamine (NH2OH) in an acidic medium to form water, nitrogen gas (N2), and oxygen gas (O2). The balanced equation for this reaction is:
2 H2O2 + 2 H+ + 2 NH2OH → 4 H2O + N2 + O2
In this reaction, hydrogen peroxide is acting as a reducing agent. It donates electrons to the hydroxylamine molecule, causing the reduction of nitrogen from the +3 oxidation state to the 0 oxidation state.
Therefore, in both reactions, hydrogen peroxide acts as a reducing agent by donating electrons to the other substances involved. It undergoes oxidation itself, resulting in the formation of oxygen gas. Hence, the correct answer is option A: reducing agent, oxidizing agent.
I. Reaction with KIO4:
Hydrogen peroxide reacts with potassium iodate (KIO4) in an acidic medium to form iodine (I2) and oxygen gas (O2). The balanced equation for this reaction is:
2 H2O2 + 2 H+ + KIO4 → I2 + K+ + 4 H2O + O2
In this reaction, hydrogen peroxide is oxidized from the -1 oxidation state to the 0 oxidation state, while KIO4 is reduced from the +7 oxidation state to the +5 oxidation state. The hydrogen peroxide donates electrons to the iodate ion, causing its reduction.
II. Reaction with NH2OH:
Hydrogen peroxide also reacts with hydroxylamine (NH2OH) in an acidic medium to form water, nitrogen gas (N2), and oxygen gas (O2). The balanced equation for this reaction is:
2 H2O2 + 2 H+ + 2 NH2OH → 4 H2O + N2 + O2
In this reaction, hydrogen peroxide is acting as a reducing agent. It donates electrons to the hydroxylamine molecule, causing the reduction of nitrogen from the +3 oxidation state to the 0 oxidation state.
Therefore, in both reactions, hydrogen peroxide acts as a reducing agent by donating electrons to the other substances involved. It undergoes oxidation itself, resulting in the formation of oxygen gas. Hence, the correct answer is option A: reducing agent, oxidizing agent.
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Hydrogen peroxide in its reaction with KIO4 and NH2OH respectively, is acting as aa)Reducing agent, oxidising agentb)Reducing agent, reducing agentc)Oxidising agent, oxidising agentd)Oxidising agent, reducing agentCorrect answer is option 'A'. Can you explain this answer?
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