Question

Xenon reacts with fluorine at \[873{\text{ }}K\]and \[7{\text{ }}bar\]to form \[{\mathbf{Xe}}{{\mathbf{F}}_4}\] ​. In this reaction the ratio of Xenon and fluorine required is :
\[{\mathbf{A}}.\;\;\;\;{\mathbf{1}}:{\mathbf{5}}\]\[B.\;\;\;\;{\mathbf{10}}:{\mathbf{1}}\]
\[C.\;\;\;\;{\mathbf{1}}:{\mathbf{3}}\]\[D.\;\;\;\;{\mathbf{5}}:{\mathbf{1}}\]

Answer 1

Hint:Xenon is a chemical element which is heavy and a rare gas of group\[{\mathbf{18}}\]. It comes under the category of noble gases and was the first noble gas found to form true chemical compounds. It is colourless, odorless and tasteless. It is a solid which has a face centred cubic crystal system and it has a single atom which behaves as spheres which are packed as closely as possible.

Complete step-by-step answer:Xenon tetrafluoride was the first discovered binary compound of a noble gas. It Is produced when xenon reacts with fluoride chemically. Being exothermic in nature, this releases an energy of \[251\;kJ/mol\]
\[{\mathbf{Xe}}{{\mathbf{F}}_4}\]is a colorless crystalline structure which can be determined by both \[NMR\]spectroscopy and \[X - \] ray crystallography. It has a square planar structure which has been confirmed by neutron diffraction studies. In addition to four fluoride ligands, the xenon centre consists of two lone pairs of electrons. This was determined by the \[VSEPR\]theory. Those lone pairs are mutually trans.
It is known to sublime at\[115.7\;^\circ C\]. its synthesis takes place by heating a mixture of xenon and fluorine in a \[1:5\]ratio in a container of nickel at a temperature of \[400^\circ C\]

Thus the correct answer is \[A\]\[1:5\].

Note:Certain amount of \[Xe{F_6}\] is formed which is called xenon hexafluoride. \[Xe{F_6}\] can be formed by the increase in concentration of fluorine. The nickel is not a catalyst for this reaction; nickel containers are used because they react with fluorine to form a protective, non-peeling layer of \[Ni{F_2}\] on their interior surfaces.