Answer to Question #100199 in General Chemistry for Beverlie

Question

At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 25.0 g H2 at 20.0°C in a 1.00 L container assuming in Part 1 non-ideal behavior and in Part 2 ideal behavior.
1. Use the van der Waals equation and data in the hint to calculate the pressure exerted. answer in atm
2. Now, calculate the pressure exerted, assuming that the gas behaves as an ideal gas. answer in atm

Answer 1

1.

Van der wall equation is-

$$(P+an^2/V^2)(V-nb)=nRT$$

Here,

$V=10^{-3}\\a=0.02067\\b=0.000015\\n=12.5\\R=8.314\\T=293K$

Putting all these values

We get,

$$(P+3229687)(0.000875)=12.5\times8.314\times293$$

$$P=31570000\ Pa=315.70\ atm$$

2.

For ideal behaviour -

$$PV=nRT\\P\times10^{-3}=12.5\times8.314\times293\\P=30450000\ Pa=304.5\ atm$$