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

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

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

= = 0.0826

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

c. heat could easily travel through the molecules in the air and escape/enter the flask. removing the air slows down the heat transfer.  

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