Question

A sample of 1.25 mol of oxygen, O2, is placed in a 5.00-L cylinder at 300 K. What is the pressure inside the container?
(R = 0.08215 L atm/mol K)
• 154 atm
• 30.8 atm
• 6.16 atm
• 0.162 atm

Answer 1

First, we need to use the ideal gas law to calculate the pressure inside the container:

PV = nRT

Where:
P = pressure
V = volume (5.00 L)
n = number of moles (1.25 mol)
R = ideal gas constant (0.08215 L atm/mol K)
T = temperature (300 K)

Now, plug in the values:

P(5.00) = (1.25)(0.08215)(300)

P(5.00) = 30.76875

P = 30.76875 / 5.00

P ≈ 6.16 atm

Therefore, the pressure inside the container is 6.16 atm. The correct answer is:
• 6.16 atm