If a cylinder contains 21.3 g of CO2 in 25.0 L at 435. 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.
To solve this problem, we can use the ideal gas law equation:
PV = nRT
where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
First, we need to convert the mass of CO2 to moles:
Molar mass of CO2 = 44.01 g/mol
Number of moles = 21.3 g / 44.01 g/mol = 0.484 moles
Now, we can plug in the values into the ideal gas law equation:
P(25.0 L) = (0.484 moles)(0.0821 L.atm/mol.K)(435 K)
P(25.0 L) = 17.658 atm
Therefore, the pressure of the CO2 in the cylinder is 17.7 atm (rounded to three significant figures).