Question

It turns out that the van der Waals constant b equals four times the total volume actually occupied by the molecules of a mole of gas.

Using this figure, calculate the fraction of the volume in a container actually occupied by Ar atoms at 230 atm pressure and 0 C. Assume b=0.0322 L/mol

Answer 1

0.0826 of the volume in the container is actually occupied by Ar atoms

Step-by-step explanation:

First we find volume occupied by 1 mole the gas using Ideal gas equation

PV = nRT

Given:

P - 230 atm

R - 0.0821 atmL/molK

T - 0 C or 273 K

n - 1

V - Vg (Volume occupied by 1 mole of gas)

Therefore,

Vg = 1 * 0.0821 * 273 / 230 = 0.09745 L

Then we find the volume actually occupied by 1 mole of Ar atoms - Va

b = 4Va

Therefore,

Va = 0.0322 / 4 = 0.00805 L

The fraction of the volume in the container actually occupied by Ar atoms is
`(Va)/(Vg)`

`(Va)/(Vg)` =
`(0.0805)/(0.09745)` = 0.0826

Therefore, 0.0826 of the volume in the container is actually occupied by Ar atoms