We can use the ideal gas law to solve this problem:
PV = nRT
where:
P = pressure = 158. atm
V = volume = 4.4 L
n = number of moles
R = ideal gas constant = 0.08206 L.atm/mol.K
T = temperature = 32 + 273.15 = 305.15 K
Plugging in the values:
(158. atm)(4.4 L) = n(0.08206 L.atm/mol.K)(305.15 K)
695.2 = n(25.0385)
n = 695.2/25.0385
n ≈ 27.73 mol
Therefore, there are approximately 27.73 moles of oxygen (O2) in the 4.4 L cylinder.
How many moles of oxygen (O2) are contained in a 4.4 L cylinder that has a pressure of 158. atm and a temperature of 32. °C? Be sure your answer has the
correct number of significant figures.
Note: Reference the Fundamental constants table for additional information.
1 answer
1 answer