Question

A compound consists of 4.50 g of nitrogen for every 7.71 g of oxygen and has the same empirical and molecular formula identify the compound

Answer 1

The compund of N2O3 has the same empirical and molecular formula when the compund consist of 4.5g of nitrogen for every 7.71 grams of oxygen.

Answer 2

Answer:

$N_2O_{3}$

Explanation:

Hi, the empirical formula is the minimal expression of the molecule composition and doesn't always represent the molecule in the reality.

On the other hand the molecular formula is a multiple of the empirical and represents how the molecule is composed in reality.

In this case they are the same.

Now, nitrogen has an atomic weight of 14 g/mol and oxygen one of 16 g/mol:

$n_{nitrogen}=\frac{4.5g}{14g/mol}$

$n_{nitrogen}= 0.321mol$

$n_{oxygen}=\frac{7.715g}{16g/mol}$

$n_{oxygen}= 0.482mol$

So the formula would be:

$N_{0.321}O_{0.482}$

Dividing per 0.321:

$NO_{1.5}$

In natural numbers:

$N_2O_{3}$