What is the molecular formula of a compound with the empirical formula of p2o3 and a gram molecular mass of 284 grams?

The answer is: the molecular formula of a compound is P₄O₁₀.

M(P₂O₅) = 2 · Ar(P) + 5 · Ar(O) · g/mol.

M(P₂O₅) = 2 · 31 + 5 · 16 · g/mol.

M(P₂O₅) = 142 g/mol; molar mass of empirical formula.

M(PₓOₙ) = 284 g/mol; molecular mass of unknown compound.

M(PₓOₙ) : M(P₂O₅) = 284 g/mol : 142 g/mol.

M(PₓOₙ) : M(P₂O₅) = 2 : 1.

answer: - 3.) the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

solution: - as per the rules, oxidation number of oxygen in its compounds is -2. the sum of oxidation numbers of all the elements of a molecule or compound is zero.

also, the oxidation number in elemental form is zero.

in no, the oxidation number of o is -2 so the oxidation number of n is +2 so that the sum is zero.

similarly, the oxidation number of c in co is +2 and o is -2.

on product side the oxidation number of n is 0 as it is in the elemental form() .

oxidation number of c in carbon dioxide is +4 as there are two oxygen in it and we know that each oxygen is -2.

so, oxidation number of n is changing from +2 to 0 and the oxidation number of c is changing from +2 to +4.

since nitrogen is reduced and hence no is acting as an oxidizing agent. carbon is oxidized and so co is acting as a reducing agent.

so, the right choice is number 3.)the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

a is the correct answer