Chapter 8, Problem 102QRT

Interpretation Introduction

Interpretation:

Number of air molecules per $c{m}^3$ remaining in the apparatus has to be calculated using the given data.

Concept Introduction:

Ideal gas Equation:

  $\text{PV = nRT}$

Where,

$P$ is the Pressure

$\text{V}$ is the Volume

$\text{n }$ is the number of moles

$\text{R}$ is the Gas constant

$\text{T}$ is the Temperature.

Molar mass can be determined using the given equation,

  $\text{n}\text{= }\frac{\text{m}}{\text{M}}$

Here, n is the number. of moles

  M is the Molar mass

    m is the Mass

Pressure can be expressed in different units.  But it is normally reported in

$\text{mm}\text{Hg}\left(\text{millimeters}\text{of}\text{mercury}\right)$

General unit conversions:

  $\begin{array}{l}\text{1}\text{Pa}\text{=}{\text{1Nm}}^{-2}{\text{ = 1 kgm}}^{-1}{s}^{-2};{\text{ 1 kPa = 10}}^{\text{3}}\text{ Pa}\\ \\ \text{1}\text{bar}\text{=}{\text{10}}^{\text{5}}{\text{Pa = 10}}^{\text{3}}{\text{ kPa; mbar = 10}}^{\text{2}}\text{ Pa}\\ \\ \text{1}\text{atm}\text{=}1.01325\times {10}^5\text{ Pa = 101}\text{.325 kPa}\\ \\ 1\text{ atm = 760 Torr = 760}\text{mm}\text{Hg}\\ \\ 1\text{ atm = 14}{\text{.7 lb/in}}^{\text{2}}\left(psi\right)\text{ = 1}\text{.01325 bar}\end{array}$