Chapter 6, Problem 6.116QE

Interpretation Introduction

Interpretation:

The pressure of $\text{1}\text{.55 mol}$ nitrogen at $530°\text{C}$ in a $3.23\text{ L}$ container has to be calculated by both the ideal gas law and the van der Waals equation has to be calculated.

Concept Introduction:

Any gas that obeys the assumption laid down in kinetic molecular theory is said to be an ideal gas. The combination of all the gas laws namely Boyle’s law, Charles law and Avogadro’s leads to the ideal gas equation that can be used to relate all the four properties such as given below:

  $PV=nRT$

Here,

$\text{R}$ is the universal gas constant.

$V$ denotes the volume.

$n$ denotes the number of moles.

$T$ denotes temperature.

$P$ denotes the pressure.

Van der Waals equation is given as follows:

  $\left(P+\frac{a{n}^2}{V^2}\right)\left(V-nb\right)=nRT$

Here,

a is a constant that gives the strength of the attractive force.

$b$ gives the measure of the size of the gas molecules.