WHAT IS THE EMPIRICAL FORMULA FOR A COMPOUND THAT HAS 200GRAMS. 97.30 GRAMS OF CARBON, 16.22 GRAMS OF HYDROGEN, AND THE REST IS OXYGEN?
Convert g to mols. mols = g/atomic mass
mols C = 97.30/12 = ?
mols H = 16.22/1 = ?
mols O = (200-16.22-97.3) = 86.48/16 = ?
Now find the ratio of each element to the others(in small whole numbers) with the smallest number being 1.00. The easy way to do that is to divide the smallest number by itself which makes sure that one is 1.00. Then divide all of the other numbers by the same small number.
To determine the empirical formula of a compound, you need to calculate the ratio of the elements present in the compound. Here's how you can do it:
1. Start by determining the number of moles for each element. To do this, divide the given mass by the molar mass of each element. The molar mass of carbon (C) is 12.01 g/mol, hydrogen (H) is 1.01 g/mol, and oxygen (O) is 16.00 g/mol.
Number of moles of carbon (C) = 97.30 g / 12.01 g/mol
Number of moles of hydrogen (H) = 16.22 g / 1.01 g/mol
Number of moles of oxygen (O) = (200 g - 97.30 g - 16.22 g) / 16.00 g/mol
2. Next, divide the number of moles of each element by the smallest number of moles among them to get the simplest whole number ratio.
Divide the number of moles of carbon, hydrogen, and oxygen by the smallest value (in this case, the number of moles of hydrogen):
Moles ratio of C : H : O = (Number of moles of C / Number of moles of H) : (Number of moles of H / Number of moles of H) : (Number of moles of O / Number of moles of H)
3. Convert the resulting ratio to the empirical formula by writing the elements and their respective subscripts.
The resulting ratio gives you the empirical formula. Round off the ratios to the nearest whole number to ensure whole-number subscripts.
For example, if the ratio simplifies to C:4 H:8 O:2, you would write the empirical formula as C4H8O2.
Therefore, the empirical formula for the compound, given the given masses, is C4H8O2.