Sodium peroxide (Na2O2) is used to remove carbon dioxide from (and add oxygen to) the air supply in spacecrafts. It works by reacting with CO2 in the air to produce sodium carbonate (Na2CO3) and O2. 2 Na2O2 (s) + 2 CO2 (g) → 2 Na2CO3 (s) + O2 (g) What volume (in liters) of CO2 can be consumed at STP by 435 g Na2O2?

The volume (in liters) of CO₂ that can be consumed at STP by 435 g Na₂O₂ is 125 L of Co₂

calculation

2Na₂O₂ (s) + 2 CO₂ (g) → 2 Na₂CO₃ (s) + O₂ (g)

Step 1 : find the moles of Na₂O₂

moles = mass: molar mass

from periodic table the molar mass of Na₂O₂ = (23 x2) + (16 x2) = 78 g/mol

moles = 435 g: 78 g/mol = 5.58 moles

Step 2: use the mole ratio to determine the moles of CO₂

from given equation Na₂O₂ : CO₂ = 2 : 2 = 1:1

Therefore the moles of CO₂ is also = 5.58 moles

Step 3: find the volume of CO₂ at STP

that is at STP 1 mole of a gas = 22.4 L

5.58 moles = ? l

by cross multiplication

= (5.58 moles x 22.4 L) / 1 mole = 125 L