Chapter 9, Problem 9.120CHP

(a)

Interpretation Introduction

Interpretation:

The molar mass of the gaseous compound $\text{Q}$ has to be calculated.

Concept Introduction:

Ideal gas equation is an equation that is describing the state of an imaginary ideal gas.

$\text{PV}\text{=}\text{n RT}$

Where,

P is the pressure of the gas

V is the volume

n is the number of moles of gas

R is the universal gas constant $\text{(R=0}{\text{.0821LatmK}}^{\text{-1}}{\text{mol}}^{\text{-1}})$

T is the temperature

Molar mass:

It is a physical property, which is defined as the mass of a given substance divided by the amount of substance. Unit of the kilogram is $\text{g/mol}$

$\text{molar mass}\text{=}\frac{\text{amount}\text{of}\text{mass}}{\text{molecular mass}}$

(b)

Interpretation Introduction

Interpretation:

The total pressure and partial pressure of $\text{Xenon}\text{and}\text{Oxygen}$ in the container has to be calculated.

Concept Introduction:

Partial Pressure:

Dalton’s law of partial pressure states that “the total pressure (P) of the mixture is equal to the sum of the partial pressures ${\text{(P}}_{\text{A}}{\text{, P}}_{\text{B}}{\text{, P}}_{\text{C}}\mathrm{.....}\text{)}$ of all the component gases $\text{(A, B, C}\mathrm{......}\text{)}$  present in the mixture” and is given as,

${\text{P = P}}_{\text{A}}{\text{ + P}}_{\text{B}}{\text{ + P}}_{\text{C}}\text{ + }\mathrm{.......}$

The ideal gas law for the individual gas component A is given as,

${\text{P}}_{\text{A}}{\text{V = n}}_{\text{A}}\text{RT}$

Mole Fraction:

$\text{The mole fraction of A = }\frac{n_{\text{A}}}{n}=\frac{{\text{P}}_{\text{A}}}{\text{P}}$