Question

A sample of oxygen gas has a density of _____ g/L at a pressure of 1.23 atm and a temperature of 35

Answer 1

Solution:

We use ideal gas equation to find out density.

Molar mass of O2 = 31.998 g/mol

Pressure = 1.23 atm

R = 0.08206 L atm / K mol

T = 35 deg C + 273.15 = 308.15 K

We know

PV = nRT

n = mole , R is gas constant , T is temperature, p is pressure , V is volume

n = m/ M , here m is in gram and M is molar mass

Lets plug value of n in ideal gas equation

PV = (m/ M )RT

Now we know density (d) = m / V

We rearrange above equation so that we get m/V to one side

m/V = PM/RT

d = PM/ RT

= (1.23 atm * 31.998 g per mol ) / (0.08206 L atm per K per mol * 308.15 K )

= 156 g/L

Density of O2 = 156 g/L