Question

What is the molecular formula of a compound if its empirical formula is $N{O_2}$ and its molar mass is $138.02g/mol$?

Answer 1

Hint: We need to know that when a synthetic recipe is a method of introducing data about the substance extents of particles that establish a specific synthetic compound or atom, utilizing compound component images, numbers, and at times likewise different images, like enclosures, runs, sections, commas and in addition to (plus) and less (minus) signs. These are restricted to a solitary typographic line of images, which may incorporate addendums and superscripts.

Complete answer:
We have to remember that a synthetic equation is certifiably not a substance name, and it contains no words. Albeit a substance equation may infer certain basic compound designs, it is not equivalent to a full synthetic underlying recipe. Compound formulae can completely determine the design of hands down the least difficult of particles and synthetic substances and are by and large more restricted in power than substance names and underlying formulae.
In the given details,
The empirical formula is $N{O_2}$ ,
The molar mass is $138.02g/mol$ ,
The molar mass of empirical formula $N{O_2}$ is $14.0g/mol$ .
First, we have to calculate the whole number, by using the following expression,
$ = \dfrac{{138.02g/mol}}{{46g/mol}} = 3$
Therefore, the whole number is three.
Now, multiplying given empirical formula, and the above whole number.
$\left( {N{O_2}} \right) \times 3 = {N_3}{O_6}$
Therefore, the molecular formula is ${N_3}{O_6}$ .

Note:
We must have to know that when a substance equation distinguishes every constituent component by its compound image and shows the proportionate number of iotas of every component. In observational formulae, these extents start with a key component and afterward allocate quantities of iotas of different components in the compound, by proportions to the key component. For subatomic mixtures, these proportion numbers would all be able to be communicated as entire numbers.