How many grams of FeS are formed from 7.62g of Fe reacted with excess S? Fe+Sarrow FeS 3.829 7.629 11.979 11.49

To determine the amount of FeS formed from 7.62g of Fe reacted with excess S, we need to use stoichiometry.<br /><br />Given information:<br />- Reaction: Fe + S → FeS<br />- Mass of Fe: 7.62g<br />- Excess S (sulfur)<br /><br />Step 1: Calculate the molar mass of Fe and FeS.<br />Molar mass of Fe = 55.85 g/mol<br />Molar mass of FeS = 87.91 g/mol<br /><br />Step 2: Calculate the moles of Fe.<br />Moles of Fe = Mass of Fe / Molar mass of Fe<br />Moles of Fe = 7.62g / 55.85 g/mol = 0.136 mol<br /><br />Step 3: Calculate the moles of FeS formed.<br />Since the reaction is 1:1, the moles of FeS formed will be the same as the moles of Fe.<br />Moles of FeS = 0.136 mol<br /><br />Step 4: Calculate the mass of FeS formed.<br />Mass of FeS = Moles of FeS × Molar mass of FeS<br />Mass of FeS = 0.136 mol × 87.91 g/mol = 11.97g<br /><br />Therefore, the correct answer is 11.97g.