Interpretation For the given pairs - reducing agent and gain of electrons, whether the concepts of pairing are correct or not have to be indicated. Concept Introduction: Reducing agent: The substance which is getting oxidized in redox reaction is the reducing agent. It will lose electrons in the reaction. Formic acid, earth metals, sulfites are examples of reducing agent. Example: Consider the reaction: N 2 +3H 2 → 2NH 3 Oxidation No of N 2 = 0 Oxidation No of H 2 = 0 Oxidation No of Nitrogen in NH 3 = -3 Oxidation No of Hydrogen in NH 3 = +1 N 2 loses electrons and H 2 gains electrons in this redox reaction. Hence H 2 is the reducing agent.
Interpretation For the given pairs - reducing agent and gain of electrons, whether the concepts of pairing are correct or not have to be indicated. Concept Introduction: Reducing agent: The substance which is getting oxidized in redox reaction is the reducing agent. It will lose electrons in the reaction. Formic acid, earth metals, sulfites are examples of reducing agent. Example: Consider the reaction: N 2 +3H 2 → 2NH 3 Oxidation No of N 2 = 0 Oxidation No of H 2 = 0 Oxidation No of Nitrogen in NH 3 = -3 Oxidation No of Hydrogen in NH 3 = +1 N 2 loses electrons and H 2 gains electrons in this redox reaction. Hence H 2 is the reducing agent.
Solution Summary: The author explains the concept of reducing agent and gain of electrons in a redox reaction.
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
Chapter 9, Problem 9.34EP
(a)
Interpretation Introduction
Interpretation
For the given pairs - reducing agent and gain of electrons, whether the concepts of pairing are correct or not have to be indicated.
Concept Introduction:
Reducing agent:
The substance which is getting oxidized in redox reaction is the reducing agent. It will lose electrons in the reaction. Formic acid, earth metals, sulfites are examples of reducing agent.
Example:
Consider the reaction:
N2+3H2→2NH3
Oxidation No of N2=0
Oxidation No of H2= 0
Oxidation No of Nitrogen in NH3= -3
Oxidation No of Hydrogen in NH3= +1
N2 loses electrons and H2 gains electrons in this redox reaction.
Hence H2 is the reducing agent.
(b)
Interpretation Introduction
Interpretation:
For the given pairs – substance oxidized and increases in oxidation number, whether the concepts of pairing are correct or not has to be indicated.
Concept Introduction:
Oxidation:
Loss of electrons from an atom ion or molecule during a chemical reaction is known as oxidation. Oxidation state of atom ion or molecule will increase in this process. In simple it is the addition of oxygen. Reduction is gaining of electrons.
Example
Here Fe2+ oxidized to Fe3+ by the removal of a single electron.
Oxidizing agent:
Oxidizing agent will gain electrons but itself will get reduced in the reaction. Oxygen, Hydrogen peroxide are good oxidizing agent.
Example:
Consider the reaction:
N2+3H2→2NH3
Oxidation No of N2=0
Oxidation No of H2= 0
Oxidation No of Nitrogen in NH3= -3
Oxidation No of Hydrogen in NH3= +1
N2 Loses electrons and H2 gains electrons in this redox reaction. Hence N2 is the oxidizing agent.
(c)
Interpretation Introduction
Interpretation
For the given pairs – oxidizing agent and gain of electrons, whether the concepts of pairing are correct or not have to be indicated.
Concept Introduction:
Oxidation:
Loss of electrons from an atom ion or molecule during a chemical reaction is known as oxidation. Oxidation state of atom ion or molecule will increase in this process. In simple it is the addition of oxygen. Reduction is gaining of electrons.
Example
Here Fe2+ oxidized to Fe3+ by the removal of a single electron.
Oxidizing agent:
Oxidizing agent will gain electrons but itself will get reduced in the reaction. Oxygen, Hydrogen peroxide are good oxidizing agent.
Example:
Consider the reaction:
N2+3H2→2NH3
Oxidation No of N2=0
Oxidation No of H2= 0
Oxidation No of Nitrogen in NH3= -3
Oxidation No of Hydrogen in NH3= +1
N2 Loses electrons and H2 gains electrons in this redox reaction. Hence N2 is the oxidizing agent.
(d)
Interpretation Introduction
Interpretation:
For the given pairs – reducing agent and substance reduced, whether the concepts of pairing are correct or not has to be indicated.
Concept Introduction:
Oxidation:
Loss of electrons from an atom ion or molecule during a chemical reaction is known as oxidation. Oxidation state of atom ion or molecule will increase in this process. In simple it is the addition of oxygen. Reduction is gaining of electrons.
Example
Here Fe2+ oxidized to Fe3+ by the removal of a single electron.
Reducing agent:
The substance which is getting oxidized in redox reaction is the reducing agent. It will lose electrons in the reaction. Formic acid, earth metals, sulfites are examples of reducing agent.
Example:
Consider the reaction:
N2+3H2→2NH3
Oxidation No of N2=0
Oxidation No of H2= 0
Oxidation No of Nitrogen in NH3= -3
Oxidation No of Hydrogen in NH3= +1
N2 Loses electrons and H2 gains electrons in this redox reaction.
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