An unknown compound with a molar mass of 223.94 g/mol consists of 32.18% c, 4.50% h, and 63.32% cl. find the molecular formula for the compound.

The actual number of atoms of each element present in the molecule of the compound is represented by the formula known as molecular formula.

Molar mass of the unknown compound = 223.94 g/mol (given)

Mass of each element present in the unknown compound is determined as:

Now, the number of each element in the unknown compound is determined by the formula:

Dividing each mole with the smallest number of mole, to determine the empirical formula:

Multiplying with 2 to convert the numbers in formula into a whole number:

So, the empirical formula is .

Empirical mass =

In order to determine the molecular formula:

n =

n =

So, the molecular formula is:

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the atomic number of carbon is six, which means that a carbon atom has six protons. carbon has three naturally occurring isotopes: carbon-12, carbon-13, and carbon-14. which of these statements are true about carbon and its isotopes? select all that appl