Chapter 8, Problem 32Q

Interpretation Introduction

Interpretation For the following statements, true statements should be found and for the false statements it should be corrected.

Concept introduction:

• Kinetic molecular theory explains the properties of ideal gas. From the postulates of kinetic molecular theory it is clear that kinetic energy of gas particle is directly proportional to the Kelvin temperature of the gas.

    Average kinetic energy of gas can be determined as,  $K{E}_{avg}=\left(3/2\right)RT$

• The average  velocity can be determined,

                                                        ${\mu }_{ave}={\left(\frac{8RT}{\pi M}\right)}^{1/2}$ (1)

        $\begin{array}{l}R=\frac{8.314J}{Kmol}\\ M=Molarmassinkg\end{array}$

• Ideal gas law tends to hold best at low pressure and high temperature

  A modified ideal gas equation on account of molecular size and molecular interaction forces is termed as Van der Waals equation.

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

‘a’ and ‘b’ is called Van der Waals coefficient and are characteristic of the   individual gas

Where,

          P = pressure in atmospheres

          V= volumes in liters

          n = number of moles

          R =universal gas constant ( $\text{0}\text{.08206L×atm/K×mol}$)

          T = temperature in kelvins

• At constant temperature and volume, the number of collision pre unit area increases by increasing the number of moles per unit area.