- You have 70% of Fe(Iron) and 30% of O(Oxygen) is the compound FeO or Fe2O3.
- Assume that one rock of Iron Oxide is 100g.
- you can than say that there is 70g of Fe and 30g of O
- next is to find the number of moles in 70g of Fe and the number of moles in O
- 70gFe= mol/Fe, 30gO= mol/O
- to figure this out you would look at the atomic mass of each element
- Fe has an atomic mass of 56 and O has an atomic mass of 16
- taking each atomic mass you divide by the number of grams
- 70/56=1.25, 30/16=1.875
- the answer will be the number mole in each element.
- 70gFe= 1.25 mol/Fe, 30gO= 1.875 mol/O
- you than take the lower number in this case 1.25 and divide 1.875 and 1.25 by 1.25
- 1.25/1.25=1, 1.875/1.25=1.5
- When you get a decimal like 1.5 you will multiply both answers by two
- 1.25/1.25=1x2=2, 1.875/1.25=1.5x2=3
- you than have your ration for every two iron there are three oxygen
- 2:3
This next problem I will not only use the empirical formula but to find the right answer when given to compounds that can work for the ratio I will than use the Molecular Formula.
Empirical Formula part 1
- YOu have 2.34g of N(Nitrogen) and 5.34g of O(Oxygen) you need to find out if this compound is No2 or N2O4? Weight is 92g/mol
- First find the number of moles in each
- 2.34gN= mol/N, 5.34gO= mol/O
- the atomic mass of N is 14 while the atomic mass of O is 16 divide the grams by the mass
- 2.34g/14=0.167, 5.34/16=0.334
- 2.34gN= 0.167 mol/N, 5.34gO= 0.334 mol/O
- divide by the lowest number(0.167)
- 0.167/0.167=1, 0.334/0.167=2
- you have a ratio of 1 nitrogen for every 2 oxygen
- 1:2
- Now find the weight simple add 16x2+14=46g/mol the weight doesn't match what we were given.
- Find out if the compound is N2O4 we have to use the molecular formula. You are given the weight of 92g/mol to get the answer you simply do the following.
- n x46=92g/mol
- 2x47=92g/mol
- answer is N2O4
Get chemistry notes from here What is empirical formula?
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