I had a question on a test that I was stumped on.
The question is:
A hydrocarbon is burned, creating CO2 and H2O.
The mass of carbon dioxide, in grams, is 3.26 times greater than the mass of water.
The molar mass of this hydrocarbon is between 50-60 g/mol.
1. What is the mass (g) of carbon in the compound?
2. What is the mass (g) of hydrogen in the compound?
3. What is the amount of moles of carbon?
4. What is the amount of moles of hydrogen?
5. What is the empirical formula?
6. What is the molecular formula?
My attempt:
I tried different ways to do it, but I don't know if they are right. They are probably wrong.
1. Knowing that the hydrocarbon's molar mass is between 50-60 g/mol, I used a guess and check method to see which possible formulas there were. I tried C4H12, as that adds up to 60 g/mol. From there I had no idea what to do.
2. I used the molar masses of H2O and tried multiplying by 3.26, however I stopped there because I also had no idea what to do
3. I tried using algebra , but I got confused:
let x =H20
(3.26x)*12/44 for the C in CO2
For the H2O, I did 2x/18
Afterwards I also had no idea what to do
There were other attempts at this but my sheet is too messy and I can't read the scribbles
If you could explain it as well without giving just the answer that'd be great
Thanks