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?
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.
To calculate the pressure inside the container, you can use the ideal gas law equation:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles
R is the ideal gas constant
T is the temperature
First, you need to find the number of moles of CO2. To do that, you can use the molar mass of CO2, which is 44.01 g/mol.
Number of moles (n) = mass / molar mass
n = 35.1 g / 44.01 g/mol
n = 0.796 mol
Next, you need to convert the volume from 4.0 L to the unit of cubic meters (m³), as the ideal gas constant (R) has units of J/(mol·K) in the SI system.
Volume (V) = 4.0 L = 0.004 m³
Now, you can substitute the values into the ideal gas law equation:
P * 0.004 m³ = 0.796 mol * 8.314 J/(mol·K) * 298 K
Simplify the equation:
P = (0.796 mol * 8.314 J/(mol·K) * 298 K) / 0.004 m³
Calculate the pressure:
P ≈ 38.8 x 10^3 Pa
Therefore, the pressure inside the container is approximately 38.8 kPa.
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.