). A sample contains 450 grams of Iron (III)sulfate. How many molecules are in this sample?

To determine the number of molecules of Iron (III) sulfate (Fe2(SO4)3) in a 450-gram sample, we need to follow these steps:1. Calculate the molar mass of Iron (III) sulfate (Fe2(SO4)3).2. Convert the mass of the sample to moles.3. Calculate the number of molecules using Avogadro's number.Step 1: Calculate the molar mass of Iron (III) sulfate (Fe2(SO4)3)Molar mass of Fe = 55.85 g/molMolar mass of S = 32.07 g/molMolar mass of O = 16.00 g/molMolar mass of Fe2(SO4)3 = (2 × 55.85) + (3 × (32.07 + 4 × 16.00))Molar mass of Fe2(SO4)3 = 399.88 g/molStep 2: Convert the mass of the sample to molesMoles of Fe2(SO4)3 = Mass of sample / Molar mass of Fe2(SO4)3Moles of Fe2(SO4)3 = 450 g / 399.88 g/molMoles of Fe2(SO4)3 ≈ 1.123 molStep 3: Calculate the number of molecules using Avogadro's numberAvogadro's number = 6.022 × 10^23 molecules/molNumber of molecules = Moles of Fe2(SO4)3 × Avogadro's numberNumber of molecules ≈ 1.123 mol × 6.022 × 10^23 molecules/molNumber of molecules ≈ 6.77 × 10^23 moleculesTherefore, there are approximately 6.77 × 10^23 molecules of Iron (III) sulfate in the 450-gram sample.