What is the empirical formula of a hydride prepared from #4*g# of hydrogen, and #28*g# of oxygen?
You know that you have 4 grams of Hydrogen and 32 grams of Oxygen in your molecule so the first step is converting both weights given into moles. You use each molecules molecular weight (1.0079 g/mol for Hydrogen and 15.999 g/mol for Oxygen) to convert between moles and grams. These values are found on a periodic table!
After you know how many moles of each compound you have, look at the ratio and see if you can reduce like you would a fraction.
This gives you your final answer!
The empirical formula is
The empirical formula is the simplest, whole number ratio defining constituent atoms in a species. And how do we get this? Well, we divide the elemental masses thru by the atomic masses of each element...........
If we divide thru by the smallest molar quantity (that of oxygen) we get