What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation?

Li + N2 ⟶ Li3 N

Li is limiting reactant

Explanation:

Based on the reaction:

6Li + N2 → 2Li3N

Where 6 moles of Li reacts per mole of N2

To solve this question we must convert the mass of each reactant to moles and using the chemical equation we can find limiting reactant

Moles Li -6.941g/mol-

1.50g * (1mol / 6.941g) = 0.2161 moles Li

Moles N2 -Molar mass:28g/mol-

1.50g * (1mol / 28g) = 0.0536 moles N2

For a complete reaction of 0.536 moles N2 are needed:

0.536 moles N2 * (6mol Li / 1mol N2) = 0.3214 moles Li

As there are just 0.2161 moles of Li

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