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.

are you sure this is correct

1 answer

Yes, to calculate the pressure of the gas in the cylinder, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = moles of gas
R = ideal gas constant
T = temperature

First, we need to calculate the moles of CO2 in the cylinder:

molar mass of CO2 = 44.01 g/mol

moles of CO2 = 40.6 g / 44.01 g/mol = 0.923 mol

Now, we can plug in the values into the ideal gas law equation:

P(27.5 L) = (0.923 mol) (0.08206 L atm/mol K) (325 K)

P(27.5 L) = 24.966 L atm

P = 24.966 L atm / 27.5 L

P = 0.909 atm

Therefore, the pressure of the CO2 gas in the cylinder at 325 K is 0.909 atm, with the correct number of significant figures.