Use the ideal gas law to calculate density
Calculate the density of oxygen gas at 788 mm Hg and 22.5 ºC.
You are asked to calculate the density of a gas at a given pressure and temperature.
You are given the identity of the gas and its pressure and temperature.
Equation 10.6 contains a constant (R = 0.082057 L·atm/K·mol), so all properties must have units that match those in the constant.
P = 788 mm Hg × \frac{1\text{ atm}}{760\text{ mm Hg}} = 1.04 atm
T = (22.5 + 273.15) K = 295.7 K
M(O_{2}) = 32.00 g/mol
Solve Equation 10.6 for density, and use it to calculate the density of oxygen under these conditions.
M = \frac{dRT}{P}
d = \frac{PM }{RT} = \frac{\left(1.04\text{ atm}\right)\left(32.00\text{ g/mol}\right) }{\left(0.082057\text{ L} \cdot \text{atm/K} \cdot \text{mol}\right) \left(295.7\text{ K}\right) } = 1.37 g/L