To solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles of gas
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature
First, we need to calculate the number of moles of CO2 in the cylinder:
n = mass / molar mass
n = 40.6 g / 44.01 g/mol (molar mass of CO2)
n = 0.923 moles
Now we can calculate the pressure using the ideal gas law equation:
P = (nRT) / V
P = (0.923 moles * 0.0821 L.atm/mol.K * 325 K) / 27.5 L
P = (23.356 L.atm/K) / 27.5 L
P = 0.850 atm
Therefore, the pressure in the cylinder is 0.850 atm. Since the volume is given to three significant figures, our answer should have three significant figures as well.
If a cylinder contains 40.6 g of CO2 in 27.5 L at 325. K, what is the pressure (in atm)? Be sure your answer has the correct number of significant figures.
Note: Reference the Fundamental constants table for additional information.
1 answer