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a compound contains carbon, hydrogen, and chlorine. it has a molar mass of 127.00 g/mol. analysis of a sample shows that it contains 37.83% carbon and 6.35% hydrogen. what is its molecular formula?



Answer :

The molecular formula of a molar mass of 127g/ mol is C9H18.

Let us assume 100g of an unknown compound.

Thus there is 37.83% × 100g/ 12.011 g[tex]mol^{-1}[/tex] concerning carbon . i.e., 3.15. mol. C

In the same manner 6.35% × 100 / 1.00794 concerning hydrogen i.e., 6.29 mol. H

Thus the empirical formula, the simplest whole number ratio that defines constituent elements is a species as CH2.

Now the molecular formula is always a whole number multiple of the empirical formula:

Empirical formula × n = molecular formula

So

( 12.011 + 2× 1.00794) ×n = 127

14.02688 × n = 127

n = 9

So the molecular formula = 9 × CH2

                                          = C9H18

Therefore the molecular formula is C9H18.

To know more about the molecular formula refer to the link given below:

https://brainly.com/question/11574373

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