Answer
1. Using the molar mass of $CO_2$ (44.01 g/mol), calculate the mass of carbon on that compound.
2. Using the molar mass of $H_2O$ (18.02 g/mol), calculate the mass of hydrogen on that compound.
3. Divide the mass of carbon by the total mass of the initial compound, and multiply by 100% to get the percent of carbon.
4. Divide the mass of hydrogen by the total mass of the initial compound, and multiply by 100% to get the percent of hydrogen.
5. Add these percents, and subtract that from 100% to find the percent of Oxygen.
6. Work with 100 g, transforming the percents directly in grams.
7. Divide each compound mass by their atomic mass, to get the amount of moles.
8. Divide them by the smallest of the three, to get the whole-number ration.
9. If it is necessary, divide them to get the smallest whole numbers, which represent the amount in the empirical formula.
Work Step by Step
1. Using the molar mass of $CO_2$ (44.01 g/mol), calculate the mass of carbon on that compound.
2. Using the molar mass of $H_2O$ (18.02 g/mol), calculate the mass of hydrogen on that compound.
3. Divide the mass of carbon by the total mass of the initial compound, and multiply by 100% to get the percent of carbon.
4. Divide the mass of hydrogen by the total mass of the initial compound, and multiply by 100% to get the percent of hydrogen.
5. Add these percents, and subtract that from 100% to find the percent of Oxygen.
6. Work with 100 g, transforming the percents directly in grams.
7. Divide each compound mass by their atomic mass, to get the amount of moles.
8. Divide them by the smallest of the three, to get the whole-number ration.
9. If it is necessary, divide them to get the smallest whole numbers, which represent the amount in the empirical formula.
