Empirical Formula 1) What is the empirical formula of a compound that contains 0.783g of Carbon 0.196g of Hydrogen and 0.521g of Oxygen?

To determine the empirical formula of the compound, we need to find the simplest whole number ratio of the moles of each element present in the compound.<br /><br />Given:<br />- Carbon (C): 0.783g<br />- Hydrogen (H): 0.196g<br />- Oxygen (O): 0.521g<br /><br />Step 1: Calculate the moles of each element.<br />Moles of Carbon (C) = 0.783g / 12.01g/mol = 0.0651 mol<br />Moles of Hydrogen (H) = 0.196g / 1.008g/mol = 0.1951 mol<br />Moles of Oxygen (O) = 0.521g / 16.00g/mol = 0.0326 mol<br /><br />Step 2: Determine the simplest whole number ratio of the moles of each element.<br />To find the simplest whole number ratio, we need to divide each mole value by the smallest mole value among the three elements.<br /><br />Ratio of Carbon (C) = 0.0651 mol / 0.0326 mol = 2<br />Ratio of Hydrogen (H) = 0.1951 mol / 0.0326 mol = 6<br />Ratio of Oxygen (O) = 0.0326 mol / 0.0326 mol = 1<br /><br />Step 3: Write the empirical formula.<br />Based on the ratios obtained in Step 2, the empirical formula of the compound is C2H6O.<br /><br />Therefore, the empirical formula of the compound that contains 0.783g of Carbon, 0.196g of Hydrogen, and 0.521g of Oxygen is C2H6O.