Question

A cylinder of O₂(g) used in breathing by patients with emphysema has a volume of 3.00 L at a pressure of 10.0 atm. If the temperature of the cylinder is 28.0 °C, what mass of oxygen is in the cylinder?

a) 1.20 g
b) 2.40 g
c) 3.60 g
d) 4.80 g

Answer 1

the mass of oxygen in the cylinder is approximately 3.87 g

To solve for the mass of oxygen in the cylinder, we can use the ideal gas law and the molar mass of oxygen.

Step-by-step explanation:

To solve this problem, we can use the ideal gas law:

PV = nRT

where

P is the pressure

V is the volume

n is the number of moles

R is the ideal gas constant

T is the temperature

We can rearrange the equation to solve for the number of moles:

n = PV / RT

Plugging in the given values:

n = (10.0 atm)(3.00 L) / (0.0821 L·atm/mol·K)(28.0 °C + 273.15)

n = 0.121 mol

To calculate the mass, we can use the molar mass of oxygen, which is 32 g/mol.

mass = n * molar mass

mass = 0.121 mol * 32 g/mol

mass = 3.87 g

Therefore, the mass of oxygen in the cylinder is approximately 3.87 g.