Chapter 13, Problem 35A

Interpretation Introduction

Interpretation: -The pressure that each gas would exert if present alone needs to be determined.

Concept Introduction: - For determining the partial pressure of the gases Dalton’s law of partial pressure is used.

According to this law,

  $\mathrm{P}=P_1+P_2+P_3$

Where

  $\begin{array}{l}{\text{P}}_{\text{T}}\text{ = Total Pressure}\text{.}\\ {\text{P}}_{\text{1}}\text{ = Partial pressure of gas A}\\ {\text{P}}_2=\text{ Partial pressure of gas B}\end{array}$

Answer to Problem 35A

Partial pressure of oxygen is $745.3Torr$ .

Explanation of Solution

The total pressure of a mixture of gases which do not react chemically is the sum of partial pressure of component gases. This is known as Dalton’s law partial pressure.

According to this law

  $\mathrm{P}=P_1+P_2$

Put the values in the formula for calculating partial pressure of ${\mathrm{O}}_2$

  $\begin{array}{c}{P}_{total}=P_{O_2}+P_{H_{2}O}\\ 772Torr=P_{O_2}+26.7Torr\\ P_{O_2}=772Torr-26.7Torr\\ P_{O_2}=745.3Torr\end{array}$

Partial pressure of Oxygen ( ${\mathrm{O}}_2$ ) = $745.3Torr$

Conclusion

Partial pressure of Oxygen ( ${\mathrm{O}}_2$ ) = $745.3Torr$