Iron reacts with sulfur , producing iron sulfide according to the chemical reaction . What is the maximum quantity (in grams) of iron sulfide produced if we use 0.5 moles of sulfur? Fe + S → FeS.

Answer 1

First, use a balanced chemical reaction equation.

FE + S → FeS is in fact balanced. It tells you that for every 1 mole of iron (Fe) and 1 mole of sulfur (S) that 1 mole of iron sulfide (FeS) is produced, So, in this case, since we start with 0.5 moles of sulfur, we will produce (assuming there is enough iron) 0.5 moles of FeS.

To convert this to grams, you must use the molar mass. To calculate the molar mass, look up iron in the periodic table and you will see the atomic mass is 55.85 g/mol and then look up sulfur and you see it has an atomic mass of 32.07 g/mol therefore FeS has a molar mass of 55.85 + 32.07 or 87.92 g/mol.

Now multiply these: (87.92 g/mol)(0.5 moles) = ? grams