Chapter 8, Problem 67QRT

Interpretation Introduction

Interpretation:

Reason for why value of $\text{PV}$ smaller than $\text{nRT}$ in ideal gas equation when pressure is increased should be explained.

Concept Introduction:

Ideal gas is the most usually used form of the ideal gas equation, which describes the relationship among the four variables P, V, n, and T.  An ideal gas is a hypothetical sample of gas whose pressure-volume-temperature behaviour is predicted accurately by the ideal gas equation.

  $\text{PV = nRT}$

Here,

  n is the moles of gas

    P is the Pressure

  V is the Volume

    T is the Temperature

    R is the gas constant

Van der Waal’s gas equation:

The van der Waal equation describes the ideal gas as it approaches to zero. The van der Waal equation contains correction terms a and b for the intermolecular forces and molecular size respectively.

The van der Waal equation is as follows,

  $\left[P+a{\left(\frac{n}{V}\right)}^2\right]\left(\frac{V}{n}-b\right)=RT$