Chapter 5.4, Problem 5.8BFP

Interpretation Introduction

Interpretation:

At $0.950\text{atm}$ of pressure and $24°\text{C}$ the density of ${\text{NO}}_2$ is to be calculated. Also, the density of ${\text{NO}}_2$ and dry air is to be compared.

Concept introduction:

Ideal gas law equation is as follows:

$PV=nRT$        (1)

Here,

$P$ is the pressure of the gas.

$V$ is the volume occupied by gas.

$n$ is the no. of moles of gas.

$T$ is the temperature in Kelvin.

$R$ is the universal gas constant.

The formula to calculate no. of moles is as follows:

$n=\frac{\text{weight}\left(m\right)}{\text{molecular}\text{weight}\left(M\right)}$

The ideal gas equation can be written as follows:

$PV=\frac{mRT}{M}$

The formula to calculate density is:

$\text{Density}=\frac{m}{V}$

The ideal gas equation can be rearranged for density as follows:

$\text{Density}=\frac{PM}{RT}$        (2)

The conversion factor to convert $°\text{C}$ to Kelvin is as follows:

$T\left(\text{K}\right)=T\left(\text{°C}\right)+273.15$        (3)