Chapter 6, Problem 104IAE

Interpretation Introduction

(a)

Interpretation:

The mass percentage of ${\text{N}}_{\text{2}}\text{O}$ gas should be calculated.

Concept introduction:

According to the Dalton’s law of partial pressure the partial pressure of any gas in the gaseous mixture is the product of mole fraction of that gas and total pressure. The mathematical expression can be written as:

Partial Pressure = Mole fraction of gas × Total Pressure

For a gaseous mixture, the average molar mass or apparent molar mass can be calculated as the sum of the mole fractions of each component gas multiplied by their molar mass. The mathematical expression can be written as:

${\text{M}}_{\text{mixture}}\text{= }\left({\text{x}}_{\text{1}}\times {\text{M}}_{\text{1}}\text{+ }\mathrm{......}{\text{+ x}}_{\text{n}}\times {\text{M}}_{\text{n}}\right)$

Here:

x_i= Mole fractions of component gas

M_i = the molar mass of component gas

Interpretation Introduction

(b)

Interpretation:

The apparent molar mass of anesthetic should be calculated.

Concept introduction:

According to the Dalton’s law of partial pressure the partial pressure of any gas in the gaseous mixture is the product of mole fraction of that gas and total pressure. The mathematical expression can be written as:

Partial Pressure = Mole fraction of gas × Total Pressure

For a gaseous mixture, the average molar mass or apparent molar mass can be calculated as the sum of the mole fractions of each component gas multiplied by their molar mass. The mathematical expression can be written as:

${\text{M}}_{\text{mixture}}\text{= }\left({\text{x}}_{\text{1}}\times {\text{M}}_{\text{1}}\text{+ }\mathrm{......}{\text{+ x}}_{\text{n}}\times {\text{M}}_{\text{n}}\right)$

Here:

x_i= Mole fractions of component gas

M_i = the molar mass of component gas