). 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:<br /><br />1. Calculate the molar mass of Iron (III) sulfate (Fe2(SO4)3).<br />2. Convert the mass of the sample to moles.<br />3. Calculate the number of molecules using Avogadro's number.<br /><br />Step 1: Calculate the molar mass of Iron (III) sulfate (Fe2(SO4)3)<br />Molar mass of Fe = 55.85 g/mol<br />Molar mass of S = 32.07 g/mol<br />Molar mass of O = 16.00 g/mol<br /><br />Molar mass of Fe2(SO4)3 = (2 × 55.85) + (3 × (32.07 + 4 × 16.00))<br />Molar mass of Fe2(SO4)3 = 399.88 g/mol<br /><br />Step 2: Convert the mass of the sample to moles<br />Moles of Fe2(SO4)3 = Mass of sample / Molar mass of Fe2(SO4)3<br />Moles of Fe2(SO4)3 = 450 g / 399.88 g/mol<br />Moles of Fe2(SO4)3 ≈ 1.123 mol<br /><br />Step 3: Calculate the number of molecules using Avogadro's number<br />Avogadro's number = 6.022 × 10^23 molecules/mol<br /><br />Number of molecules = Moles of Fe2(SO4)3 × Avogadro's number<br />Number of molecules ≈ 1.123 mol × 6.022 × 10^23 molecules/mol<br />Number of molecules ≈ 6.77 × 10^23 molecules<br /><br />Therefore, there are approximately 6.77 × 10^23 molecules of Iron (III) sulfate in the 450-gram sample.