A .4791 g sample was analyzed and found to contain the following masses of elements:
carbon, .1929 g
hydrogen, .01079 g
oxygen, .08566 g
chlorine .1898 g
Determine the empirical formula of the new compound.
Never mind, I figured out how to do the problem.
To determine the empirical formula of a compound, we need to find the ratio of the elements present in the compound.
Step 1: Calculate the number of moles for each element.
To do this, divide the mass of each element by their respective molar masses.
- Carbon: 0.1929 g / 12.01 g/mol = 0.01607 mol
- Hydrogen: 0.01079 g / 1.008 g/mol = 0.0107 mol
- Oxygen: 0.08566 g / 16 g/mol = 0.00535 mol
- Chlorine: 0.1898 g / 35.45 g/mol = 0.00536 mol
Step 2: Find the smallest mole value.
In this case, the smallest mole value is 0.00535 mol (oxygen).
Step 3: Divide each mole value by the smallest value.
Dividing each mole value by 0.00535 mol gives us:
- Carbon: 0.01607 mol / 0.00535 mol = 3
- Hydrogen: 0.0107 mol / 0.00535 mol = 2
- Oxygen: 0.00535 mol /0.00535 mol = 1
- Chlorine: 0.00536 mol / 0.00535 mol = 1
Step 4: Simplify the ratio, if possible.
Since all the values are already whole numbers, there is no need for further simplification.
Step 5: Write the empirical formula.
Based on the ratio obtained in Step 3, the empirical formula of the compound is C3H2OCl.
Therefore, the empirical formula of the new compound is C3H2OCl.