A) \[Xe{{F}_{4}}+{{O}_{2}}{{F}_{2}}\xrightarrow{{}}Xe{{F}_{6}}+{{O}_{2}}\]
B) \[Xe{{F}_{2}}+P{{F}_{5}}\xrightarrow{{}}{{[XeF]}^{+}}+PF_{6}^{-}\]
C) \[Xe{{F}_{6}}+P{{F}_{5}}\xrightarrow{{}}XeO{{F}_{4}}+2HF\]
D) \[Xe{{F}_{6}}+2{{H}_{2}}O\xrightarrow{{}}Xe{{O}_{2}}{{F}_{2}}+4HF\]
Correct Answer: A
Solution :
| The reaction in which oxidation and reduction occurs simultaneously are Termed as redox reaction or where there is change in oxidation number on both reactants and product sides. |
| [a] \[(\overset{+\,4}{\mathop{X}}\,){{F}_{4}}+{{\overset{+\,1}{\mathop{O}}\,}_{2}}({{F}_{2}})\xrightarrow{{}}{{\overset{+\,6}{\mathop{X}}\,}_{e}}{{F}_{6}}+{{\overset{0}{\mathop{O}}\,}_{2}}\] |
| Since, Xe undergoes oxidation while O undergoes reduction. So, it is an example of redox reaction. |
| [b] \[({{\overset{+\,4}{\mathop{X}}\,}_{e}}){{F}_{2}}+\overset{+\,5}{\mathop{P{{F}_{5}}}}\,\xrightarrow{{}}{{\overset{+\,6}{\mathop{[X}}\,}_{e}}F{{]}^{+}}\overset{+\,5}{\mathop{P{{F}_{6}}}}\,\] |
| As the oxidation state of P is same on both sides. Thus, it is not a redox reaction. |
| [c] \[\overset{+\,6}{\mathop{X}}\,e{{F}_{6}}+{{H}_{2}}O\xrightarrow{{}}\overset{+\,6}{\mathop{X}}\,e{{F}_{4}}\] |
| Not a redox reaction. |
| [d] \[\overset{+\,6}{\mathop{X}}\,e{{F}_{6}}+2{{H}_{2}}O\xrightarrow{{}}\overset{+\,6}{\mathop{X}}\,e{{O}_{2}}{{F}_{2}}+4HF\] |
| Not a redox reaction. |
You need to login to perform this action.
You will be redirected in
3 sec
