How many moles of an ideal gas are there in a container with a pressure of 108,893 Pa, a temperature of 321 K

How many moles of an ideal gas are there in a container with a pressure of 108,893 Pa,
a temperature of 321 K, and a volume of 2.0 L? The universal gas constant is 8.314
J/Kmol.


The answer is 0.082 mol
Can someone please show me the steps, Thank you so much.

This is a straightforward application of the Ideal Gas Law:

PV = nRT

P = pressure
V = volume
n = number of moles
R = universal gas constant
T = absolute temperature

The only 'trick' is a units conversion. Just recall that:
Pa = N/m²; J = N•m
and you can quickly verify that
Pa•m³ = N•m = J
And recall that L = 10˜³ m³

Solve for n:
n = PV/RT = 1.08893*10⁵ * 2.0*10˜³ / (8.314 * 321) Pa•m³/(K•J/K•mol)
= 8.16*10˜² mol
= 0.082 mol, to 2 significant figures, since that's the level of the least precise input (2.0 L).