Question

Dry ice is simply frozen carbon dioxide (carbon dioxide in the solid state) and is pretty cold with a temperature of -109.3 degrees F (-78.5 degrees C). For comparison, liquid nitrogen is MUCH colder at -321 degrees Fahrenheit (-196 degrees Celsius). The carbon dioxide in dry ice will also go directly from the solid state (frozen carbon dioxide) to the gaseous state

You have 2.44 grams of dry ice in a 6.0 Liter container maintained at 31.2O C. What is the pressure in the container after ALL the dry ice has sublimated (transformed to the gaseous state)?

Answer 1

Pressure in container = 0.23 atm       (exact pressure = 0.23083 atm)

Explanation

Mass of dry ice (solid CO₂) = 2.44 g

molar mass of CO₂ = 44.0 g/mol

moles of CO₂ = mass / molar mass = 2.44 g / (44.0 g/mol)

moles of CO₂ = 0.0555 mol

Volume of container = 6.0 L

Temperature = 31.2 ^oC = (31.2 + 273 K) = 304.2 K

According to ideal gas law, P = (n * R * T) / V

where P = pressure of CO₂

R = gas constant = 0.0821 L-atm/mol-K

P = (0.0555 mol * 0.0821 L-atm/mol-K * 304.2 K) / 6.0 L

P = 0.23 atm