Question

Dry ice (solid carbon dioxide) has a density of 1.35 g/mL. If 25.0 mL of dry ice is placed inside an empty balloon and completely sublimes to gaseous carbon dioxide, then what is the balloon’s volume at STP? Assume the balloon was sealed after the solid CO₂ was added.

How many moles of CO₂_22​(g) are present after 25.0 mL of dry ice sublimes?

Answer 1

The volume of a balloon at STP after 25.0 mL of dry ice sublimes is approximately 17.2 liters, and the sublimation produces about 0.767 moles of CO₂ gas.

Step-by-step explanation:

The student asks what volume a balloon will occupy at STP conditions when 25.0 mL of dry ice sublimes completely into a gaseous state and how many moles of CO₂ gas are present. Using the density of dry ice, which is 1.35 g/mL, we first calculate the mass of 25.0 mL of dry ice:

Mass = 25.0 mL × 1.35 g/mL = 33.75 g

Next, we use the molar mass of CO₂ (44.01 g/mol) to find the moles of CO₂:

Moles of CO₂ = Mass / Molar mass = 33.75 g / 44.01 g/mol ≈ 0.767 moles of CO₂

Since one mole of a gas at STP occupies 22.4 L, we can find the volume the balloon will occupy:

Volume at STP = Moles of CO₂ × Volume per mole at STP = 0.767 moles × 22.4 L/mol ≈ 17.2 L

Therefore, the volume of the balloon at STP after the dry ice sublimes is approximately 17.2 liters, and there are about 0.767 moles of CO₂ gas present.