Consider the following reaction:
4NaO₂(s) + 2CO₂(g) $\rightarrow$ 2Na₂CO₃(s) + 3O₂(g)
How many moles of NaO₂ are needed to react with 75.0 L of carbon dioxide at STP?

Question

Consider the following reaction:
4NaO₂(s) + 2CO₂(g)

\rightarrow

2Na₂CO₃(s) + 3O₂(g)
How many moles of NaO₂ are needed to react with 75.0 L of carbon dioxide at STP?

Quizplus · Accepted Answer

At STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.4 L. Therefore, 75.0 L of CO2 corresponds to $75.0 \, \text{L} \div 22.4 \, \text{L/mol} = 3.35 \, \text{moles of CO2}$. According to the balanced chemical equation, 2 moles of CO2 react with 4 moles of Na2O, so the moles of Na2O needed are $3.35 \, \text{moles CO2} \times \frac{4 \, \text{moles Na2O}}{2 \, \text{moles CO2}} = 6.70 \, \text{moles Na2O}$.

Consider the Following Reaction: 4NaO2(s)+ 2CO2(g) →\rightarrow→ 2Na2CO3(s)+ 3O2(g) How Many Moles of NaO2 Are Needed

Consider the Following Reaction:
4NaO₂(s)+ 2CO₂(g) $\rightarrow$ 2Na₂CO₃(s)+ 3O₂(g)
How Many Moles of NaO₂ Are Needed