Question

What is the density(in g/L) of a gas with a molar mass of 32.49g/mol at 2.569atm and 458K?

Answer 1

Answer:

$2.22~g/L$

Explanation:

According to the ideal gas law equation:

$pV = nRT$

Let's express the number of moles in terms of mass and molar mass:

$pV = \frac{m}{M} RT$

Let's divide both sides by volume:

$p = \frac{m}{MV} RT$

Notice that:

$\frac{m}{V} = d$

So the equation becomes:

$p = \frac{dRT}{M}$

Expressing density:

$d = \frac{pM}{RT}$

Substituting the given values:

$d = \frac{2.569~atm\cdot 32.49~g/mol}{0.08206~\frac{L~atm}{mol~K}\cdot 458~K} = 2.22~g/L$