Chapter 1, Problem 1A.4ST

Interpretation Introduction

Interpretation:

The partial pressures of a sample of gas consisting of $\text{2}\text{.50 g}$ oxygen and $\text{6}\text{.43 g}$ of carbon dioxide with a total pressure of $\text{88 kPa}$  has to be calculated.

Concept Introduction:

Mole fractions:

The number of moles of sample id divided by total mole to give mole fraction of sample that present in given mixture.

For example, mole fraction of A in AB mixture is,

    $\begin{array}{l}{\text{x}}_{\text{A}}\text{=}\frac{{\text{n}}_{\text{A}}}{{\text{n}}_{\text{A}}{\text{+n}}_{\text{B}}}\\ \text{Where,}\\ {\text{x}}_{\text{A}}\text{-}\text{mole}\text{fraction}\text{of}\text{A}\\ {\text{n}}_{\text{A}}\text{-}\text{number}\text{of}\text{mole}\text{of}\text{A}\\ {\text{n}}_{\text{B}}\text{-}\text{number}\text{of}\text{mole}\text{of}\text{B}\end{array}$

Partial pressure:

The pressure for the each individual gas to contributing the total pressure for gaseous mixture is known as partial pressure.

For example, partial pressure for A in AB gaseous mixture is,

    $\begin{array}{l}{\text{p}}_{\text{A}}\text{=}{\text{x}}_{\text{A}}{\text{×P}}_{\text{t}}\\ \text{Where,}\\ {\text{p}}_{\text{A}}\text{-}\text{partial pressure}\text{for}\text{A}\\ {\text{x}}_{\text{A}}\text{-}\text{mole}\text{fraction}\text{of}\text{A}\\ {\text{P}}_{\text{t}}\text{-}\text{total}\text{pressure}\end{array}$