Final answer:
To find the theoretical yield of lithium nitride in the reaction of lithium with nitrogen, convert the mass of each reagent to moles, identify the limiting reactant based on the molar ratios, and calculate the maximum amount of lithium nitride that can be produced according to the stoichiometry of the balanced equation.
Step-by-step explanation:
To determine the theoretical yield of lithium nitride from the given reaction, we need to consider the stoichiometry of the reaction. The balanced chemical equation for the reaction between lithium (Li) and nitrogen (N2) to form lithium nitride (Li3N) is:
6Li(s) + N2(g) → 2Li3N(s)
Since the question provides us with 3.00g samples of each reagent, we must first convert these masses to moles to use the molar ratio from the balanced equation:
- Amount of Li in moles = mass / molar mass of Li = 3.00g / 6.94g/mol
- Amount of N2 in moles = mass / molar mass of N2 = 3.00g / 28.02g/mol
Next, we will identify the limiting reactant by comparing the mole ratio of the reactants to the stoichiometry of the balanced equation. The reactant that gives the fewer moles of product is the limiting reactant, and this determines the maximum amount of product that can be formed.
Following the stoichiometry, for every 6 moles of Li reacted, 2 moles of Li3N are produced. We will calculate the amount of Li3N that could be produced from each reactant, assuming the other is in excess. The one that produces the lesser amount of Li3N will be the theoretical yield.