The reaction of ${P_4}$ with X leads selectively to ${P_4}{O_6}$. The X is : a.) dry ${O_2}$ b.) a mixture of ${O_2}$ and ${N_2}$ c.) moist ${O_2}$ d.) ${O_2}$ in presence of aq. NaOH
Answer
Verified
Hint: This reaction requires less supply of oxygen. So, some other element will be used that will competitively inhibit the full supply of oxygen.
Complete step by step answer: For this, first, we will see the reaction of formation of ${P_4}{O_6}$. ${P_4} + 3{O_2}\xrightarrow[{{N_2}}]{{{O_2}}}{P_4}{O_6}$ Phosphorus trioxide is prepared by heating phosphorus in a limited supply of oxygen and nitrogen. Oxygen supply is provided in a limited quantity because if it is in more quantity then ${P_4}{O_6}$ will further oxidize to ${P_4}{O_6}$.
Thus, option b.) is the correct answer.
Additional information: Phosphorus exists in two major forms – white phosphorus and red phosphorus. Phosphorus is highly reactive. So, it is never found as a free element. Many oxides of phosphorus are formed in nature. Phosphorus trioxide is a colourless solid. It is the anhydride of phosphoric acid. So, in reaction with water, we get phosphorous acid. It is a good ligand for transition metals. Further, low temperature is required during its formation. Phosphorus trioxide is found to have a tetrahedral point group. This was determined from electron diffraction data. It consists of P – O – P bonds as well.
Note: Nitrogen when present along with oxygen limits its supply so that further oxidation can be prevented. Absence of nitrogen will give a complete supply of oxygen and this can lead to oxidation of the product further.
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