The density of oxygen gas at 298 K and 1 atm is closest to?

To find the density of oxygen gas at 298 K and 1 atm, we can use the ideal gas law, which states that PV = nRT.

Here, P = pressure = 1 atm V = volume n = number of moles R = ideal gas constant = 0.0821 L atm / (mol K) T = temperature = 298 K

We want to find the density, which is mass/volume. We know that one mole of oxygen gas (O2) has a mass of approximately 32 g. So, we can rewrite the equation as follows:

PV = (mass/RMM)RT

where RMM is the relative molecular mass.

Rearranging for mass/volume (density), we get:

Density = PM/RT

Substituting the known values:

Density = (1 atm * 32 g/mol) / (0.0821 L atm / (mol K) * 298 K)

Solving this gives a density of approximately 1.43 g/L.