Question

Suppose that we continue to work with the gas from the previous problem ( 2 moles of gas occupy 126 L at 346 K, and that the van der Waals constants are a = 6.20 atmL^2/mol^2 and b = 0.0852 L/mol), but consider the molecules to be mathematical points. Calculate the pressure and compare it to the values from the previous problem.

Answer 1

0.448 atm

Step-by-step explanation:

So, we have;

n = 2 moles

V = 126 L

T = 346 K

a = 6.20 atmL^2/mol^2

b = 0.0852 L/mol

R = 0.082 atmLK-1mol-1

P = nRT/V -nb - an^2/V^2

Substituting values;

P=2 * 0.082 * 346/126 -(2 * 0.0852) - 6.20 * 2^2/126^2

P=56.744/125.8296 -24.8/15876

P= 0.45 - 0.001562

P= 0.448 atm