Problem: 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:Assume b= 0.0322 L/mol.at 200 atm pressure and 0 oC. (Assume for simplicity that the ideal-gas equation still holds.) 

🤓 Based on our data, we think this question is relevant for Professor All Professors' class at LSU.

FREE Expert Solution

Concept: van der Waals equation.

Using the b constant for Ar gas, find the initial volume of Ar gas. 

Next use the ideal gas law to solve for the volume at T= 0°C and P = 200 atm.

View Complete Written Solution
Problem Details

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:
Assume b= 0.0322 L/mol.

at 200 atm pressure and 0 oC. (Assume for simplicity that the ideal-gas equation still holds.)