Question

Which of the following reactions is an example of a redox reaction?
A. ${\rm{Xe}}{{\rm{F}}_{\rm{2}}} + {\rm{P}}{{\rm{F}}_{\rm{5}}} \to {\left[ {{\rm{XeF}}} \right]^{\rm{ + }}} + {\rm{P}}{{\rm{F}}_{\rm{6}}}^ -$
B. ${\rm{Xe}}{{\rm{F}}_{\rm{6}}} + {{\rm{H}}_2}{\rm{O}} \to {\rm{XeO}}{{\rm{F}}_4} + {\rm{2HF}}$
C. ${\rm{Xe}}{{\rm{F}}_6} + {\rm{2}}{{\rm{H}}_2}{\rm{O}} \to {\rm{Xe}}{{\rm{O}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}} + 4{\rm{HF}}$
D. ${\rm{Xe}}{{\rm{F}}_{\rm{4}}} + {{\rm{O}}_2}{{\rm{F}}_2} \to {\rm{Xe}}{{\rm{F}}_6} + {{\rm{O}}_{\rm{2}}}$

Answer 1

We know that the redox reaction is one of those sorts of reactions in which the reduction and oxidation generally take place simultaneously or at the same time. The redox reaction is one of the abbreviations used for reduction and oxidation reaction.

Complete solution
As we all know, in the oxidation reaction, the oxidation state of the species increases gradually. In contrast, in the reduction chemical reaction, the oxidation state of any given species decreases gradually.
In other words, the gaining or addition of electrons from other species in the given chemical reaction by any element, then this element is said to be a reduced element and the reaction is a reduction reaction. Similarly, the losing or dropping of electrons from any other species in the given chemical reaction by an element, then this element is said to be an oxidized element and the reaction is an oxidation reaction.
The oxidation state elements in option A is $\mathop {{\rm{Xe}}}\limits^{ + 2} \mathop {{{\rm{F}}_{\rm{2}}}}\limits^{ - 1} + \mathop {\rm{P}}\limits^{ + 5} \mathop {{{\rm{F}}_{\rm{5}}}}\limits^{ - 1} \to$ $[XeF]^- \, + {PF_6}^-$
The oxidation state elements in option B is $\mathop {{\rm{Xe}}}\limits^{ + 6} \mathop {{{\rm{F}}_{\rm{6}}}}\limits^{ - 1} + \mathop {{{\rm{H}}_2}}\limits^{ + 1} \mathop {\rm{O}}\limits^{ - 2} \to \mathop {{\rm{Xe}}}\limits^{ + 6} \mathop {\rm{O}}\limits^{ - 2} \mathop {{{\rm{F}}_4}}\limits^{ - 1} + {\rm{2}}\mathop {\rm{H}}\limits^{ + 1} \mathop {\rm{F}}\limits^{ - 1}$.
The oxidation state elements in option C is$\mathop {{\rm{Xe}}}\limits^{ + 6} \mathop {{{\rm{F}}_{\rm{6}}}}\limits^{ - 1} + {\rm{2}}\mathop {{{\rm{H}}_2}}\limits^{ + 1} \mathop {\rm{O}}\limits^{ - 2} \to \mathop {{\rm{Xe}}}\limits^{ + 6} {\mathop {\rm{O}}\limits^{ - 2} _{\rm{2}}}{\mathop {\rm{F}}\limits^{ - 1} _{\rm{2}}} + 4\mathop {\rm{H}}\limits^{ + 1} \mathop {\rm{F}}\limits^{ - 1}$.
The oxidation state elements in option D is $\mathop {{\rm{Xe}}}\limits^{ + 4} \mathop {{{\rm{F}}_{\rm{4}}}}\limits^{ - 1} + \mathop {{{\rm{O}}_2}}\limits^{ + 1} \mathop {{{\rm{F}}_2}}\limits^{ - 1} \to \mathop {{\rm{Xe}}}\limits^{ + 6} \mathop {{{\rm{F}}_6}}\limits^{ - 1} + \mathop {{{\rm{O}}_{\rm{2}}}}\limits^0$.

In option D, the oxidation state of xenon gradually increases from $+ 4$ to $+ 6$. Hence, the given species xenon gets oxidized, and the oxidation of oxygen in the option D decreases gradually from $+ 1$ to $0$. Hence, the given species oxygen gets reduced.
So, in option D, both oxidation and reduction act at the same time, then this is a suitable example of a redox reaction.

**Therefore, the correct option for this given question is (D).

Note: **
The electrochemical cell, which generally is used in our daily life is usually based on the application redox reaction.