In the following reaction, how many grams of ferrous sulfide will produce 0.56 grams of iron oxide?
4FeS+7O2->2Fe2O3+4SO2
The molar mass of ferrous sulfide is 87.92 grams and that of iron oxide is 159.7
Write and balance the equation.
Convert 0.56 g Fe2O3 to mols. mols = g/molar mass.
Convert mols Fe2O3 to mols FeS using the coefficients in the balanced equation.
Then convert mols FeS to grams. g = mols x molar mass.
the equation says that 4 moles of FeS produce 2 moles of Fe2O3.
So, you use twice as many moles of FeS as you get in Fe2O3.
So, how many moles of Fe2O3 is .56g?
Use twice that many moles of FeS, then convert that into grams.
To find out how many grams of ferrous sulfide will produce 0.56 grams of iron oxide, we need to use the balanced chemical equation and convert the given mass of iron oxide to the moles of iron oxide, and then use the stoichiometry of the reaction to find the moles of ferrous sulfide.
Step 1: Convert grams of iron oxide to moles of iron oxide
Given: Mass of iron oxide = 0.56 grams
Molar mass of iron oxide (Fe2O3) = 159.7 g/mol
Using the formula:
moles of iron oxide = mass of iron oxide / molar mass of iron oxide
moles of iron oxide = 0.56 g / (159.7 g/mol) = 0.003509 mol
Step 2: Use the stoichiometry of the reaction to find moles of ferrous sulfide
From the balanced chemical equation:
4FeS + 7O2 -> 2Fe2O3 + 4SO2
The stoichiometric ratio between ferrous sulfide (FeS) and iron oxide (Fe2O3) is 4:2 or 2:1. This means that for every 2 moles of iron oxide produced, 1 mole of ferrous sulfide is required.
moles of ferrous sulfide = moles of iron oxide / 2
moles of ferrous sulfide = 0.003509 mol / 2 = 0.001755 mol
Step 3: Convert moles of ferrous sulfide to grams of ferrous sulfide
Molar mass of ferrous sulfide (FeS) = 87.92 g/mol
Using the formula:
mass of ferrous sulfide = moles of ferrous sulfide * molar mass of ferrous sulfide
mass of ferrous sulfide = 0.001755 mol * 87.92 g/mol = 0.154 grams
Therefore, 0.56 grams of iron oxide will produce approximately 0.154 grams of ferrous sulfide.