Question

In the following reaction:
${A^ + } + B \to A + {B^ + }$ oxidizing agent is:
A. ${A^ + }$
B. $B$
C. Both of them
D. None of the them

Answer 1

Hint: We can define redox reactions as chemical reactions in which transfer of electrons takes place between two reactants. Oxidation states of the species will change by the transfer of electrons that are reacting. The redox reactions take place in Batteries or electrochemical cells.

Complete step by step answer:
The given chemical equation is,
${A^ + } + B \to A + {B^ + }$
As we know that the loss of electron leads to oxidation process while the gain of electron leads to the reduction reaction.
Oxidizing agents are that species (molecule/ion) that accepts electrons and reducing agents are species (molecule/ion) that donates electrons. A substance that is oxidized acts as a reducing agent and substance that is reduced acts as oxidizing agent.
An oxidizing agent (or) an oxidant is a chemical species, which has a tendency to oxidize other substances; it leads to an increase in the oxidation state of the substance by losing electrons.
We can write oxidation half reaction as,
$B \to {B^ + } + {e^ - }$
We can write reduction half reaction as,
${A^ + } + {e^ - } \to A$
We can see that substance $B$ gets oxidized to ${B^ + }$ and it is the reducing agent.
Substance ${A^ + }$ gets reduced to $A$ and it is an oxidizing agent.
So the oxidizing agent for this reaction is ${A^ + }$.

Therefore, the option (A) is correct.

Note:
Some of the common examples of oxidizing agents are oxygen, halogens and hydrogen peroxide. Some of the industrial applications of oxidizing agents are,
Bleaching of fabrics
Combustion of fuel includes the use of oxidizing agents.
Energy storage in batteries.
Water purification.
Rubber vulcanization.
Used in biological processes like photosynthesis and metabolism.