Question

P5 roblem 10.41- Enhanced-with Feedback ?) 5of17 (> Part A A 32 7 g sanple of solid C0 (dry ce) s added toa contansr at a temperature of 100 K with a volume of 50L You may want to reference (Pages 404 401) Section 10 4 ehle completing this problem If the container is evacuated (al of thea emoved) sealed and then allowed to warm to room temperature T 258 K so that all of the sold CO converted ? a gas, what iste pressie nsde the contarer? xpress your answer to two significant figures and inchade the appropriate unts PValue Units Provide Fee

Answer 1

Ans. # Moles of CO₂ =Mass / MW = 32.7 g / (44.01 g/ mol) = 0.743 mol

# At 100K, all CO₂ is in solid state. When the container is evacuated, no CO₂ is lost because it’s in solid state. Further increasing the temperature to 298 K converts all solid CO₂ in gaseous phase.

So, the pressure in the vessel is solely due to pressure of CO₂ gas.

# Use ideal gas equation to calculate the pressure as follow-

Ideal Gas equation : PV = nRT -Equation 1 Pressure in atm where, P = V = Volume in liters nNumber of moles R = 0.0821 atm L mol-1 K-1 T = Temperature in kelvin Given, 5.00 L 298 K 0.743 mol n = Putting the values in equation 1 0.743 mol x 0.0821 atm L mol Kx 298 K 5.00 L Hence, P 3.64 atm