Consider the following generic reaction: $$\mathrm{Y}_{2}+2 \mathrm{XY} \longrightarrow 2 \mathrm{XY}_{2}$$ In a limiting reactant problem, a certain quantity of each reactant is given and you are usually asked to calculate the mass of product formed. If \(10.0 \mathrm{g}\) of \(\mathrm{Y}_{2}\) is reacted with \(10.0 \mathrm{g}\) of \(\mathrm{XY}\) outline two methods you could use to determine which reactant is limiting (runs out first) and thus determines the mass of product formed.

Two methods can be used to determine the limiting reactant and the mass of the product formed. Method 1: Comparing moles of reactants 1. Calculate molar masses of Y2 and XY. 2. Convert given grams to moles for each reactant. 3. Determine the mole ratio of reactants. 4. Divide moles of each reactant by the stoichiometric coefficients. 5. The reactant with the smallest value is the limiting reactant. 6. Use the limiting reactant's moles to calculate moles of product formed. 7. Calculate the mass of the product formed by multiplying the moles of the product by the molar mass of the product. Method 2: Comparing masses of reactants 1. Calculate molar masses of Y2 and XY. 2. Determine the mass ratio of reactants. 3. Calculate the mass of Y2 required to completely react with the given mass of XY. 4. Compare the actual mass of Y2 with the calculated mass of Y2 required to react. 5. The reactant requiring the smallest amount of the other reactant to completely react is the limiting reactant. 6. Use the mass of the limiting reactant and the mass ratio to determine the mass of the product formed.