A 35.1g sample of solid CO2 (dry ice) is added to a container at a temperature of 100k with a volume of 4.0L. If the container is evacuated (all of the gas removed), sealed and then allowed to warm to room temperature (T=298K) so that all of the solid CO2 is converted to a gas, what is the pressure inside the container?
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Help me please? Answer is 4.9atm
The sublimation point of CO2 is about -80 C (at 1 atm pressure) so I assume the problem intends for there to be no vaporization as the container is evacuated.
If we make that assumption then use PV = nRT with n = 35.1 grams/molar mass CO2 = ? The T you use is 298.
If we make that assumption then use PV = nRT with n = 35.1 grams/molar mass CO2 = ? The T you use is 298.
Use given information and plug into PV=nRT, solve for P. Then take P (from PV=nRT) and use P1/T1=P2/T2 to solve for P2.
2 answers