15.3: Gases and Pressure
Lesson Objectives
The student will:
 define pressure.
 convert requested pressure units.
 read barometers and open and closedend manometers.
Vocabulary
 atmosphere
 barometer
 manometer
 pascal
 torr
Introduction
As you learned earlier, gases exert a pressure on their surroundings. The pressure is a result of trillions of tiny particles pounding on a surface. This section will define pressure in more details, as well as explore the different ways that pressure is measured.
Pressure
Pressure is defined as the force exerted divided by the area over which the force is exerted:



\begin{align*}\text{Pressure} = \frac {\text{Force}} {\text{Area}}\end{align*}
Pressure=ForceArea

\begin{align*}\text{Pressure} = \frac {\text{Force}} {\text{Area}}\end{align*}

The concept of force is quite straightforward. Force can be described as a push or pull that causes an object to change its velocity or to change shape. Pressure, however, is a little trickier to understand. Let's consider an example that will illustrate the concept of pressure. Consider the large man and the smaller woman shown in the figure below.
The man weighs \begin{align*}200\ \mathrm{pounds}\end{align*}



\begin{align*}\text{Pressure} = \frac {\text{Force}} {\text{Area}} = \frac {200. \ \text{pounds}} {4.0 \ \text{inches}^2} = 50. \ \text{lbs}/\text{in}^2\end{align*}
Pressure=ForceArea=200. pounds4.0 inches2=50. lbs/in2

\begin{align*}\text{Pressure} = \frac {\text{Force}} {\text{Area}} = \frac {200. \ \text{pounds}} {4.0 \ \text{inches}^2} = 50. \ \text{lbs}/\text{in}^2\end{align*}

The woman, on the other hand, weighs only \begin{align*}100 \ \mathrm{pounds}\end{align*}



\begin{align*}\text{Pressure} = \frac {\text{Force}} {\text{Area}} = \frac {100. \ \text{pounds}} {0.250 \ \text{inches}^2} = 400. \ \text{lbs}/\text{in}^2\end{align*}
Pressure=ForceArea=100. pounds0.250 inches2=400. lbs/in2

\begin{align*}\text{Pressure} = \frac {\text{Force}} {\text{Area}} = \frac {100. \ \text{pounds}} {0.250 \ \text{inches}^2} = 400. \ \text{lbs}/\text{in}^2\end{align*}

This huge pressure has little to do with her weight and more to do with the area of her shoe heels. If these two people attempted to walk across the lawn, the 200pound man would likely have no problem, whereas the 100pound woman may run into trouble and have her heels sink into the grass. Pressure is not just about the total force exerted, but also about the area over which it exerted. This is the reason that nails and tent pegs are sharpened on the end. If the end were blunt, the force exerted by a hammer would be insufficient to generate enough pressure to cause the object to be pounded into a piece of wood or the ground.
Atmospheric Pressure
The tremendous pressure that can be exerted by gaseous molecules was once demonstrated by a German physicist named Otto von Guericke, who was the inventor of the air pump. Von Guericke placed two hemispheres about the size of dinner plates together and pumped the air out from between them. Before pumping, the pounding of molecules on both sides of the hemispheres is balanced. When the air between the hemispheres is removed, however, there are no air molecules on the inside of the hemispheres to balance the pounding of air molecules on the outside. As a result, there are only air molecules on the the outside pushing the hemispheres together. The force holding the two hemispheres is so strong, teams of horses were unable to pull the hemispheres apart. When von Guericke opened a valve and allowed air back inside, he could easily separate the hemispheres by hand.
The air molecules in our atmosphere exert pressure on every surface they contact. The air pressure of our atmosphere at sea level is approximately \begin{align*}15 \ \mathrm{lbs/in}^2\end{align*}
An empty glass tube with one end opened and the other end closed was completely filled with liquid mercury. The dish was also filled twothirds of the way full with mercury. The open end of the tube was covered by a finger before it was inverted and submerged into the dish of mercury. Since the open end was covered, no air could get into the tube. When the finger was removed, the mercury in the tube fell to a height such that the difference between the surface of the mercury in the dish and the top of the mercury column in the tube was \begin{align*}760\ \mathrm{millimeters.}\end{align*}
The reason why mercury stays in the tube is because there are air molecules pounding on the surface of the mercury in the dish but not on the top of the mercury in the tube. The volume of empty space in the tube is a vacuum, so there are no air molecules available to exert a balancing pressure. The weight of the mercury in the tube divided by the area of the opening in the tube is exactly equal to the atmospheric pressure. The diameter of the tube makes no difference in determining the atmospheric pressure because doubling the diameter of the tube doubles the volume of mercury in the tube and the weight of the mercury. It also doubles the area over which the force is exerted, so the pressure will be the same for all tubes. No matter the size of the tube you might choose, the air pressure will hold the mercury to the same height.
The height to which the mercury is held would only be \begin{align*}760.\ \mathrm{millimeters}\end{align*}
Measuring Gas Pressure
There are many different units for measuring and expressing gas pressure. You will need to be familiar with most of them so that you can convert between them easily. Because instruments for measuring pressure often contain a column of mercury, the most commonly used units for pressure are based on the height of the mercury column that the gas can support. As a result, one unit for gas pressure is \begin{align*}\mathrm{mm \ of \ Hg}\end{align*}



\begin{align*}1.00\ \text{atm} = 760.\ \text{mm of Hg} = 760.\ \text{torr}\end{align*}
1.00 atm=760. mm of Hg=760. torr

\begin{align*}1.00\ \text{atm} = 760.\ \text{mm of Hg} = 760.\ \text{torr}\end{align*}

Recall that pressure is defined as force divided by area. In physics, force is expressed in a unit called newton (N), and area is expressed in meters^{2} (m^{2}). Therefore, pressure in physics is expressed in \begin{align*}\mathrm{Newtons/meter}^2\end{align*}



\begin{align*}1.00\ \text{atm} = 101,325\ \text{N/m}^2 = 101,325\ \text{Pa} = 760\ \text{mm of Hg} = 760\ \text{torr}\end{align*}
1.00 atm=101,325 N/m2=101,325 Pa=760 mm of Hg=760 torr

\begin{align*}1.00\ \text{atm} = 101,325\ \text{N/m}^2 = 101,325\ \text{Pa} = 760\ \text{mm of Hg} = 760\ \text{torr}\end{align*}

As it happens, one Pascal is an extremely small pressure, so it is convenient to use kilopascals (kPa) when expressing gas pressure. Therefore, \begin{align*}1.00\ \mathrm{atm}= 101.325\ \mathrm{kPa}\end{align*}
Example:
Convert \begin{align*}425\ \mathrm{torr}\end{align*}
Solution:
The conversion factor is \begin{align*}760.\ \mathrm{torr} = 1.00\ \mathrm{atm}\end{align*}


 \begin{align*}(425\ \text{torr}) \cdot \left (\frac {1.00\ \text{atm}} {760.\ \text{torr}}\right ) = 0.559\ \text{atm}\end{align*}

Example:
Convert \begin{align*}425\ \mathrm{torr}\end{align*} to \begin{align*}\mathrm{kPa}\end{align*}.
Solution:
The conversion factor is \begin{align*}760.\ \mathrm{torr} = 101.325\ \mathrm{kPa}\end{align*}.


 \begin{align*}(425\ \text{torr}) \cdot \left (\frac {101.325\ \text{kPa}} {760.\ \text{torr}}\right ) = 56.7\ \text{kPa}\end{align*}

Example:
Convert \begin{align*}0.500\ \mathrm{atm}\end{align*} to \begin{align*}\mathrm{mm}\end{align*} of \begin{align*}\mathrm{Hg}\end{align*}.
Solution:
The conversion factor is \begin{align*}1.00\ \mathrm{atm}= 760.\ \mathrm{mm}\end{align*} of \begin{align*}\mathrm{Hg}\end{align*}.


 \begin{align*}(0.500\ \text{atm}) \cdot \left (\frac {760.\ \text{mm of Hg}} {1.00\ \text{atm}}\right ) = 380.\ \text{mm of Hg}\end{align*}

Example:
Convert \begin{align*}0.500\ \mathrm{atm}\end{align*} to \begin{align*}\mathrm{kPa}\end{align*}.
Solution:
The conversion factor is \begin{align*}1.00\ \mathrm{atm}= 101.325\ \mathrm{kPa}\end{align*}.


 \begin{align*}(0.500\ \text{atm}) \cdot \left (\frac {101.325\ \text{kPa}} {1.00\ \text{atm}}\right ) = 50.7\ \text{kPa}\end{align*}

You might notice that if you want to measure a gas pressure around \begin{align*}2.0\ \mathrm{atm}\end{align*} with a barometer, you would need a glass column filled with mercury that was over \begin{align*}1.5\ \mathrm{meters}\end{align*} high. That would be a fragile and dangerous instrument, as mercury fumes are toxic. If we used water (which is onethirteenth as dense as mercury) instead, the column would have to be \begin{align*}50\ \mathrm{feet}\end{align*} high. As a more practical alternative, instruments called manometers have been designed to measure gas pressure in flasks. There are two kinds of manometers used: openend manometers and closedend manometers.
We will look at closedend manometers (illustrated below) first, as they are easier to read. As indicated in the diagram below, the empty space above the mercury level in the tube is a vacuum. Therefore, there are no molecules pounding on the surface of the mercury in the tube. In manometer A, the flask does not contain any gas, so there are no molecules to exert a pressure. In other words, \begin{align*}\text{P}_{gas} = 0\end{align*}. The mercury level in the outside arm balances the mercury level in the inside arm, so the two mercury levels will be exactly even.
We let the flask of manometer B contain a gas at \begin{align*}1.00\ \mathrm{atm}\end{align*} pressure. The mercury level in the outside tube (the arm further from the flask) will rise to a height of \begin{align*}760\ \mathrm{mm \ of \ Hg}\end{align*}. The excess mercury in the outside tube balances the gas pressure in the flask. In manometer C, we would read the gas pressure in the flask as \begin{align*}200.\ \mathrm{mm \ of \ Hg}\end{align*}. In closedend manometers, the excess mercury is always in the outside tube, and the height difference in mercury levels will equal the gas pressure in the flask.
In the openend manometers illustrated below, the openend of the tube allows atmospheric pressure to push down on the top of the column of mercury. In manometer A, the pressure inside the flask is equal to atmospheric pressure. The two columns of mercury balance each other, so they are at the same height. Therefore, the atmospheric pressure pushing on the outside column of mercury must equal the gas pressure in the flask pushing on the inside column of mercury.
In order to properly read an openend manometer, you must know the actual air pressure in the room because atmospheric pressure is not always \begin{align*}760\ \mathrm{mm \ of \ Hg}\end{align*}. In manometer B, the pressure inside the flask balances the atmospheric pressure plus an additional pressure of \begin{align*}300.\ \mathrm{mm \ of \ Hg}\end{align*}. If the actual atmospheric pressure is \begin{align*}750.\ \mathrm{mm \ of \ Hg}\end{align*}, then the pressure in the flask is \begin{align*}1050\ \mathrm{mm \ of \ Hg}\end{align*}. On the other hand, the pressure in the flask of manometer C is less than atmospheric pressure, so the excess mercury is in the inside arm of the manometer (the arm closer to the flask). If atmospheric pressure is \begin{align*}750.\ \mathrm{mm \ of \ Hg}\end{align*}, then the pressure in the flask is \begin{align*}650.\ \mathrm{mm \ of \ Hg}\end{align*}. For openend manometers, when the excess mercury is in the outside arm, the height difference is added to atmospheric pressure. When excess mercury is in the inside arm, the height difference is subtracted from atmospheric pressure.
Scientists also use mechanical pressure gauges on occasion. These instruments use the stretching or compression of springs to turn dials, or something similar. While such instruments seem to be less trouble, they must all be calibrated against mercury column instruments and are more susceptible to reactive gases.
Lesson Summary
 Pressure is defined as the force exerted divided by the area over which the force is exerted: \begin{align*}\text{Pressure} = \frac {\text{Force}} {\text{Area}}\end{align*}.
 The air molecules in our atmosphere exert pressure on every surface they contact.
 There are many different units for measuring and expressing gas pressure, including mm of Hg, torr, atmosphere (atm), and pascal (Pa).
 At sea level, atmospheric pressure is approximately \begin{align*}15 \ \mathrm{lbs/in}^2\end{align*}, \begin{align*}760 \ \mathrm{mm \ of \ Hg}\end{align*}, \begin{align*}760 \ \mathrm{torr}\end{align*}, \begin{align*}1 \ \mathrm{atm}\end{align*}, and \begin{align*}101,325 \ \mathrm{Pa}\end{align*}.
 The barometer is a device to measure atmospheric pressure that consists of a glass tube filled with liquid mercury placed in a dish of mercury.
 A manometer is designed to measure gas pressure in flasks.
 There are two kinds of manometers: an openend manometer and a closedend manometer.
Further Reading / Supplemental Links
This video provides an introduction to gases and gas pressure.
Review Questions
 The manometer shown is a closedend manometer filled with mercury. If the atmospheric pressure in the room is \begin{align*}760.\ \mathrm{mm \ of \ Hg}\end{align*} and \begin{align*}\triangle h\end{align*} is \begin{align*}65\ \mathrm{mm \ of \ Hg}\end{align*}, what is the pressure in the flask?
 The manometer shown is a closedend manometer filled with mercury. If the atmospheric pressure in the room is \begin{align*}750.\ \mathrm{mm \ of \ Hg}\end{align*} and \begin{align*}\triangle h\end{align*} is \begin{align*}0\ \mathrm{mm \ of \ Hg}\end{align*}, what is the pressure in the flask?
 The manometer shown is an openend manometer filled with mercury. If the atmospheric pressure in the room is \begin{align*}750.\ \mathrm{mm \ of \ Hg}\end{align*} and \begin{align*}\triangle h\end{align*} is \begin{align*}65\ \mathrm{mm \ of \ Hg}\end{align*}, what is the pressure in the flask?
 The manometer shown is an openend manometer filled with mercury. If the atmospheric pressure in the room is \begin{align*}760.\ \mathrm{mm \ of \ Hg}\end{align*} and \begin{align*}\triangle h\end{align*} is \begin{align*}0\ \mathrm{mm \ of \ Hg}\end{align*}, what is the pressure in the flask?
 Explain why at constant volume, the pressure of a gas decreases by half when its Kelvin temperature is reduced by half.