Featured Answer is a community of 2,548,719 amazing learners

We're a place where learners ask for help for their tasks and share their knowledge.

Need help with a chemistry Question?

A hydrocarbon is burnt completely in air to form 17.6g of carbon dioxide gas and 7.2g of water.

What is the molecular formula of the hydrocarbon compound?

I don wan to know the answer, please tell me how to do it

There will be the same number of moles of C and H on both sides of the equation, so all the Carbon in your original hydrocarbon is now present in CO2, and all H is in the H2O.

Hydrogen

Calculate moles of H in H2O

molar mass H2O = 16.00 + (2 x 1.008) = 18.016 g/mol

molar mass H = 1.008 g/mol

moles = mass / molar mass

moles H2O = 0.002560 g / 18.016 g/mol

= 1.421 x 10^-4 moles of H2O

In ever H2O there are 2 moles of H

therefore moles of H in H2O, and thus in your original hydrocarbon = 2 x 1.421 x 10^-4

= 2.842 x 10^-4 moles of H

Carbon

Calculate moles C in CO2

molar mass CO2 = (16.00 x 2) + 12.01 = 44.01 g/mol

moles CO2 = mass / molar mass = 0.012507 g / 44.01 g/mol

= 2.842 x 10^-4 moles of CO2

Every CO2 molecule has 1 Carbon, therefore moles of C in CO2 and thus in the original hydrocarbon

= 2.842 x 10^-4 moles of C

Now work out the ratio of C : H

C : H

= 2.842 x 10^-4 : 2.842 x 10^-4

To get it into whole number divide both numbers in the ratio by the lowest number (both here are the same, but this will not always be the case

C : H

= (2.842 x 10^-4 / 2.842 x 10^-4) : (2.842 x 10^-4 / 2.842 x 10^-4)

= 1:1

So empirical formula is CH