To determine the empirical formula of the compound, we will follow these steps:1. Assume that we have 100 grams of the compound. This means we have 29.5 grams of sodium Na , 41.1 grams of sulfur S , and 29.4 grams of oxygen O .2. Convert the mass of each element to moles by dividing by their respective atomic masses.3. Divide each mole value by the smallest mole value to get the mole ratio.4. Round the mole ratio to the nearest whole number to get the empirical formula.Step 1:Mass of Na = 29.5 gMass of S = 41.1 gMass of O = 29.4 gStep 2:Moles of Na = 29.5 g / 22.99 g/mol atomic mass of Na = 1.283 molesMoles of S = 41.1 g / 32.07 g/mol atomic mass of S = 1.281 molesMoles of O = 29.4 g / 16.00 g/mol atomic mass of O = 1.838 molesStep 3:Divide each mole value by the smallest mole value 1.281 moles :Mole ratio of Na = 1.283 / 1.281 1Mole ratio of S = 1.281 / 1.281 1Mole ratio of O = 1.838 / 1.281 1.4Step 4:Since the mole ratio of O is not close to a whole number, we can try multiplying all the mole ratios by a small whole number to see if we can get whole numbers. Let's try multiplying by 2:Mole ratio of Na = 1 * 2 = 2Mole ratio of S = 1 * 2 = 2Mole ratio of O = 1.4 * 2 = 2.8 3Now we have whole numbers for the mole ratios. So, the empirical formula of the compound is Na2S2O3.