Lithium oxide can be produced by the reaction shown below.If a manufacturing company wants to make 25.0 g of Li₂O,what mass of Li is necessary? [Molar masses: Li,6.94 g/mol; O,16.00 g/mol] 4Li(s)+ O₂(g)→ 2Li₂O(s)

Question

Quizplus · Accepted Answer

First, calculate the molar mass of $Li_2O$: $2 \times 6.94 + 16.00 = 29.88 \, \text{g/mol}$. To produce 25.0 g of $Li_2O$, we use the ratio from the balanced equation, which shows 4 moles of Li are needed to produce 2 moles of $Li_2O$. Thus, for 25.0 g of $Li_2O$, the moles of $Li_2O$ are $25.0 \, \text{g} / 29.88 \, \text{g/mol} = 0.8367 \, \text{moles}$. Since 2 moles of $Li_2O$ require 4 moles of Li, 0.8367 moles of $Li_2O$ require $0.8367 \times 2 = 1.6734$ moles of Li. The mass of Li required is $1.6734 \, \text{moles} \times 6.94 \, \text{g/mol} = 11.6 \, \text{g}$.

Lithium Oxide Can Be Produced by the Reaction Shown Below