Final answer:
In the combination of 1.50 g of lithium and 1.50 g of nitrogen to form lithium nitride, lithium is the limiting reactant because the amount of lithium present is insufficient for complete reaction with the available nitrogen based on the stoichiometry of the balanced equation.
Step-by-step explanation:
To determine the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, we follow these steps:
Balance the chemical equation: 6Li + N₂ → 2Li₃N.
Calculate the molar mass of each reactant.
Determine the number of moles of each reactant based on the given mass.
Use the stoichiometry of the balanced equation to compare the mole ratio of the reactants to identify the limiting reactant.
Molar mass of Li = 6.94 g/mol. Moles of Li = 1.50 g / 6.94 g/mol = 0.216 mol.
Molar mass of N₂ = 28.02 g/mol. Moles of N₂ = 1.50 g / 28.02 g/mol = 0.054 mol.
According to the balanced equation, 6 moles of Li react with 1 mole of N₂. Therefore, to react with 0.054 mol of N₂, you would need 0.054 mol x 6 = 0.324 mol of Li, but only 0.216 mol of Li is available.
Since Li is needed in a greater quantity and the available amount is less than required, lithium is the limiting reactant. Therefore, the answer is a) Lithium is the limiting reactant.