A solvent is found to be 50.0% oxygen, 37.5% carbon, and 12.5% hydrogen. What is the empirical mass of the said compound in g/mol?Use:C = 12 amuH = 1 amuO = 16 amu

To find the empirical mass of the compound, we first need to convert the percentages into grams (since the molecular weight is expressed in grams/mole).

Assuming we have 100g of the compound, the mass of each element would be:

• Oxygen: 50.0g
• Carbon: 37.5g
• Hydrogen: 12.5g

Next, we convert the mass of each element to moles using the atomic masses given:

• Oxygen: 50.0g / 16g/mol = 3.125 mol
• Carbon: 37.5g / 12g/mol = 3.125 mol
• Hydrogen: 12.5g / 1g/mol = 12.5 mol

The empirical formula is the ratio of the number of atoms of each element in the compound. To find this, we divide each number of moles by the smallest number of moles calculated:

• Oxygen: 3.125 mol / 3.125 = 1
• Carbon: 3.125 mol / 3.125 = 1
• Hydrogen: 12.5 mol / 3.125 = 4

So, the empirical formula of the compound is CH4O.

Finally, to find the empirical mass, we add up the atomic masses of the atoms in the empirical formula:

• Carbon: 1 * 12g/mol = 12g/mol
• Hydrogen: 4 * 1g/mol = 4g/mol
• Oxygen: 1 * 16g/mol = 16g/mol

Adding these together gives an empirical mass of 32g/mol.