12.1 Gas Pressure

Learning Objectives

By the end of this section, you will be able to:

  • Define the property of pressure
  • Define and convert among the units of pressure measurements
  • Describe the operation of common tools for measuring gas pressure
  • Calculate pressure from manometer data

The earth’s atmosphere exerts a pressure, as does any other gas. Although we do not normally notice atmospheric pressure, we are sensitive to pressure changes—for example, when your ears “pop” during take-off and landing while flying, or when you dive underwater. Gas pressure is caused by the force exerted by gas molecules colliding with the surfaces of objects (Figure 12.1a). Although the force of each collision is very small, any surface of appreciable area experiences a large number of collisions in a short time, which can result in a high pressure. In fact, normal air pressure is strong enough to crush a metal container when not balanced by equal pressure from inside the container.

The left side of this figure includes a graphic of the earth with an inverted rectangular prism extending from a point on it. Near the top of the image, the label, “square inch column of air molecules” is connected to the prism with a line segment. This label is also connected with a line segment to a downward pointing arrow at the right side of the figure. Beneath the arrow is a red circle labeled, “atmospheric pressure.” A narrow rectangle with a dashed line border extends from the bottom of the arrow vertically through the circle. Directly beneath this rectangle at the lower edge of the circle is a hand with a thumb appearing to be resting on a tabletop. The thumb is connected with a line segment to the label, “14.7 lbs of pressure on 1 square inch.” The red circle is sitting on top of the thumb.
Figure 12.1a The atmosphere above us exerts a large pressure on objects at the surface of the earth, roughly equal to the weight of a bowling ball pressing on an area the size of a human thumbnail (credit: Chemistry (OpenStax),CC BY 4.0).

Watch Railroad tank car vacuum implosion (1 min)

Video source: Tom Brattain. (2008, September 29). Railroad tank car vacuum implosion [Video]. YouTube.

Watch Crush a 55 gallon drum with air pressure (4 mins)

Video source: Imagination Station Toledo. (2012, February 22). Crush a 55 gallon drum with air pressure [Video]. YouTube.

Atmospheric pressure is caused by the weight of the column of air molecules in the atmosphere above an object, such as the tanker car. At sea level, this pressure is roughly the same as that exerted by a full-grown African elephant standing on a doormat, or a typical bowling ball resting on your thumbnail. These may seem like huge amounts, and they are, but life on earth has evolved under such atmospheric pressure. If you actually perch a bowling ball on your thumbnail, the pressure experienced is twice the usual pressure, and the sensation is unpleasant.

In general, pressure is defined as the force exerted on a given area: [latex]P = \frac{F}{A}[/latex]. Note that pressure is directly proportional to force and inversely proportional to area. Thus, pressure can be increased either by increasing the amount of force or by decreasing the area over which it is applied; pressure can be decreased by decreasing the force or increasing the area.

Let’s apply this concept to determine which would be more likely to fall through thin ice in Figure 12.1b—the elephant or the figure skater? A large African elephant can weigh 7 tons, supported on four feet, each with a diameter of about 1.5 ft (footprint area of 250 in2), so the pressure exerted by each foot is about 14 lb/in2:

[latex]\text{pressure per elephant foot} = 14,000 \frac{\text{lb}}{\text{elephant}} \times \frac{1 \;\text{elephant}}{4 \;\text{feet}} \times \frac{1 \;\text{foot}}{250 \;\text{in}^2} = 14 \;\text{lb/in}^2[/latex]

The figure skater weighs about 120 lbs, supported on two skate blades, each with an area of about 2 in2, so the pressure exerted by each blade is about 30 lb/in2:

[latex]\text{pressure per skate blade} = 120 \frac{\text{lb}}{\text{skater}} \times \frac{1 \;\text{skater}}{2 \;\text{blades}} \times \frac{1 \;\text{blade}}{2 \;\text{in}^2} = 30 \;\text{lb/in}^2[/latex]

Even though the elephant is more than one hundred times heavier than the skater, it exerts less than one-half of the pressure and would therefore be less likely to fall though thin ice. On the other hand, if the skater removes her skates and stands with bare feet (or regular footwear) on the ice, the larger area over which her weight is applied greatly reduces the pressure exerted:

[latex]\text{pressure per human foot} = 120 \frac{\text{lb}}{\text{skater}} \times \frac{1 \;\text{skater}}{2 \;\text{feet}} \times \frac{1 \;\text{foot}}{30 \;\text{in}^2} = 2 \;\text{lb/in}^2[/latex]
A photo of a large gray elephant on grassy, beige terrain is pictured beside a photo of a figure skater with her right skate on the ice, upper torso lowered, arms extended upward behind her chest, and left leg extended upward behind her.
Figure 12.1b Although (a) an elephant’s weight is large, creating a very large force on the ground, (b) the figure skater exerts a much higher pressure on the ice due to the small surface area of her skates. (credit a: modification of work by Guido da Rozze, CC BY 2.0; credit b: modification of work by Ryosuke Yagi, CC BY 2.0)

Watch Describing the invisible properties of gas – Brian Bennett (4 mins)

Video source: TED-Ed. (2012b, October 10). Describing the invisible properties of gas – Brian Bennett [Video]. YouTube.

Exercise 12.1a

Practice using the following PhET simulation: Gases Intro

Activity source: Simulation by PhET Interactive Simulations, University of Colorado Boulder, licensed under CC-BY-4.0

The SI unit of pressure is the pascal (Pa), with 1 Pa = 1 N/m2, where N is the newton, a unit of force defined as 1 kg m/s2. One pascal is a small pressure; in many cases, it is more convenient to use units of kilopascal (1 kPa = 1000 Pa) or bar (1 bar = 100,000 Pa). In the United States, pressure is often measured in pounds of force on an area of one square inch—pounds per square inch (psi)—for example, in car tires. Pressure can also be measured using the unit atmosphere (atm), which originally represented the average sea level air pressure at the approximate latitude of Paris (45°). Table 12.1a provides some information on these and a few other common units for pressure measurements

Table 12.1a  Pressure Units
Unit Name and Abbreviation Definition or Relation to Other Unit
pascal (Pa) 1 Pa = 1 N/m2

recommended IUPAC unit
kilopascal (kPa) 1 kPa = 1000 Pa
pounds per square inch (psi) air pressure at sea level is ~14.7 psi
atmosphere (atm) 1 atm = 101,325 Pa

air pressure at sea level is ~1 atm
bar (bar, or b) 1 bar = 100,000 Pa (exactly)

commonly used in meteorology
millibar (mbar, or mb) 1000 mbar = 1 bar
inches of mercury (in. Hg) 1 in. Hg = 3386 Pa

used by aviation industry, also some weather reports
torr [latex]1 \;\text{torr} = \frac{1}{760} \;\text{atm}[/latex]

named after Evangelista Torricelli, inventor of the barometer
millimeters of mercury (mm Hg) 1 mm Hg ~1 torr

Exercise 12.1b

Check Your Learning Exercise (Text Version)

Canadian tire pressure gauges are marked in units of kilopascals. The reading on this type of pressure gauge for 32 psi will be

Check Your Answer[1]

Source: “Exercise 12.1b” is adapted from “Exercise 8.1-7” in General Chemistry 1 & 2, a derivative of Chemistry (Open Stax) by Paul Flowers, Klaus Theopold, Richard Langley & William R. Robinson, licensed under CC BY 4.0.

Example 12.1a

Conversion of Pressure Units

The United States National Weather Service reports pressure in both inches of Hg and millibars. Convert a pressure of 29.2 in. Hg into:

  1. torr
  2. atm
  3. kPa
  4. mbar

Solution

This is a unit conversion problem. The relationships between the various pressure units are given in Table 12.1a.

  1. [latex]29.2 \;\rule[0.5ex]{2.2em}{0.1ex}\hspace{-2.2em}\text{in Hg} \times \frac{25.4 \;\rule[0.25ex]{1.2em}{0.1ex}\hspace{-1.2em}\text{mm}}{1 \;\rule[0.25ex]{0.6em}{0.1ex}\hspace{-0.6em}\text{in}} \times \frac{1 \;\text{torr}}{1 \;\rule[0.25ex]{2em}{0.1ex}\hspace{-2em}\text{mm Hg}} = 742 \;\text{torr}[/latex]
  2. [latex]742 \;\rule[0.5ex]{1.8em}{0.1ex}\hspace{-1.8em}\text{torr} \times \frac{1 \;\text{atm}}{760 \;\rule[0.25ex]{1.2em}{0.1ex}\hspace{-1.2em}\text{torr}} = 0.976 \;\text{atm}[/latex]
  3. [latex]742 \;\rule[0.5ex]{1.8em}{0.1ex}\hspace{-1.8em}\text{torr} \times \frac{101.325 \;\text{kPa}}{760 \;\rule[0.25ex]{1.0em}{0.1ex}\hspace{-1.0em}\text{torr}} = 98.9 \;\text{kPa}[/latex]
  4. [latex]98.9 \;\rule[0.5ex]{1.9em}{0.1ex}\hspace{-1.9em}\text{kPa} \times \frac{1000 \;\rule[0.25ex]{0.9em}{0.1ex}\hspace{-0.9em}\text{Pa}}{1 \;\rule[0.25ex]{1.1em}{0.1ex}\hspace{-1.1em}\text{kPa}} \times \frac{1 \;\rule[0.25ex]{0.9em}{0.1ex}\hspace{-0.9em}\text{bar}}{100,000 \;\rule[0.25ex]{1.0em}{0.1ex}\hspace{-1.0em}\text{Pa}} \times \frac{1000 \;\text{mbar}}{1 \;\rule[0.25ex]{1.0em}{0.1ex}\hspace{-1.0em}\text{bar}} = 989 \;\text{mbar}[/latex]

Exercise 12.1c

A typical barometric pressure in Kansas City is 740 torr. What is this pressure in atmospheres, in millimetres of mercury, in kilopascals, and in bar?

Check Your Answer[2]

We can measure atmospheric pressure, the force exerted by the atmosphere on the earth’s surface, with a barometer (Figure 12.1d). A barometer is a glass tube that is closed at one end, filled with a nonvolatile liquid such as mercury, and then inverted and immersed in a container of that liquid. The atmosphere exerts pressure on the liquid outside the tube, the column of liquid exerts pressure inside the tube, and the pressure at the liquid surface is the same inside and outside the tube. The height of the liquid in the tube is therefore proportional to the pressure exerted by the atmosphere.

This figure shows two barometers. The barometer to the left contains a shallow reservoir, or open container, of mercury. A narrow tube extends upward from the reservoir above the reservoir. This tube is sealed at the top. To the right, a second similar setup is shown with a reservoir filled with water. Line segments connect the label “vacuum” to the tops of the two narrow tubes. The tube on the left shows the mercury in the reservoir extending in a column upward in the narrow tube. Similarly, the tube on the right shows the water in the reservoir extending upward into the related narrow tube. Double-headed arrows extend from the surface of each liquid in the reservoir to the top of the liquid in each tube. A narrow column or bar extends from the surface of the reservoir to the same height. This bar is labeled “atmospheric pressure.” The level of the water in its tube is significantly higher than the level of mercury in its tube.
Figure 12.1d In a barometer, the height, h, of the column of liquid is used as a measurement of the air pressure. Using very dense liquid mercury (left) permits the construction of reasonably sized barometers, whereas using water (right) would require a barometer more than 30 feet tall (credit: Chemistry (OpenStax),CC BY 4.0).

If the liquid is water, normal atmospheric pressure will support a column of water over 10 meters high, which is rather inconvenient for making (and reading) a barometer. Because mercury (Hg) is about 13.6-times denser than water, a mercury barometer only needs to be [latex]\frac{1}{13.6}[/latex] as tall as a water barometer—a more suitable size. Standard atmospheric pressure of 1 atm at sea level (101,325 Pa) corresponds to a column of mercury that is about 760 mm (29.92 in.) high. The torr was originally intended to be a unit equal to one millimetre of mercury, but it no longer corresponds exactly. The pressure exerted by a fluid due to gravity is known as hydrostatic pressure, p:

[latex]p = h\rho g[/latex]

where h is the height of the fluid, ρ is the density of the fluid, and g is acceleration due to gravity.

Exercise 12.1d

Check Your Learning Exercise (Text Version)

Why should you roll or belly-crawl rather than walk across a thinly-frozen pond?

Check Your Answer[3]

Source: “Exercise 12.1b” is adapted from “Exercise 8.1-3” in General Chemistry 1 & 2, a derivative of Chemistry (Open Stax) by Paul Flowers, Klaus Theopold, Richard Langley & William R. Robinson, licensed under CC BY 4.0.

Example 12.1b

Calculation of Barometric Pressure

Show the calculation supporting the claim that atmospheric pressure near sea level corresponds to the pressure exerted by a column of mercury that is about 760 mm high. The density of mercury = 13.6 g/cm3.

Solution

The hydrostatic pressure is given by p = hρg, with h = 760 mm, ρ = 13.6 g/cm3, and g = 9.81 m/s2. Plugging these values into the equation and doing the necessary unit conversions will give us the value we seek. (Note: We are expecting to find a pressure of ~101,325 Pa:)

[latex]101,325 N/ \text{m}^2 = 101,325 \frac{\text{kg} \cdot \text{m/s}^2}{\text{m}^2} = 101,325 \frac{\text{kg}}{\text{m} \cdot \text{s}^2}[/latex]
[latex]\begin{array}{l @{{}={}}l} p & = (760 \;\text{mm} \times \frac{1 \;\text{m}}{1000 \;\text{mm}}) \times (\frac{13.6 \;\text{g}}{1 \;\text{cm}^3} \times \frac{1 \;\text{kg}}{1000 \;\text{g}} \times \frac{(100 \;\text{cm})^3}{(1 \;\text{m})^3}) \times (\frac{9.81 \;\text{m}}{1 \;\text{s}^2}) \\[1em] & = (0.760 \;\text{m}) (13,600 \;\text{kg/m}^3) (9.81 \;\text{m/s}^2) = 1.01 \times 10^5 \;\text{kg/ms}^2 = 1.01 \times 10^5 \;N/ \text{m}^2 \\[1em] & = 1.01 \times 10^5 \;\text{Pa} \end{array}[/latex]

Exercise 12.1e

Calculate the height of a column of water at 25 °C that corresponds to normal atmospheric pressure. The density of water at this temperature is 1.0 g/cm3.

Check Your Answer[4]

Exercise 12.1f

Check Your Learning Exercise (Text Version)

A typical barometric pressure in Denver, Colorado, is 615 mm Hg. What is this pressure in atmospheres and kilopascals?

Check Your Answer[5]

Source: “Exercise 12.1f” is adapted from “Exercise 8.1-5” in General Chemistry 1 & 2, a derivative of Chemistry (Open Stax) by Paul Flowers, Klaus Theopold, Richard Langley & William R. Robinson, licensed under CC BY 4.0.

A manometer is a device similar to a barometer that can be used to measure the pressure of a gas trapped in a container. A closed-end manometer is a U-shaped tube with one closed arm, one arm that connects to the gas to be measured, and a nonvolatile liquid (usually mercury) in between. As with a barometer, the distance between the liquid levels in the two arms of the tube (h in the diagram) is proportional to the pressure of the gas in the container. An open-end manometer (Figure 12.1e) is the same as a closed-end manometer, but one of its arms is open to the atmosphere. In this case, the distance between the liquid levels corresponds to the difference in pressure between the gas in the container and the atmosphere.

Three diagrams of manometers are shown. Each manometer consists of a spherical pink container filled with gas on the left that is connected to a U-shaped, sealed tube by a valve on its right. The top of the U-shape aligns with the gas-filled sphere and the U, which extends below, contains mercury. The first manometer has a sealed tube. The sealed end to the upper right in the diagram is labeled “closed end” and “vacuum.” An arrow points downward in the left side of the U shaped tube to the mercury surface. This arrow is labeled “P subscript gas.” The mercury level is higher in the right side of the tube than in the left. The difference in height is labeled “h.” Beneath this manometer illustration appears the label P subscript gas equal sign h rho g. The second manometer has an open ended tube, which is labeled “open end.” At this opening in the upper right of the diagram is a downward arrow, above which is the label P subscript a t m. An arrow points downward in the left side of the U shaped tube to the mercury surface. This arrow is labeled “P subscript gas.” The mercury level is higher in the left side of the tube than in the right. This difference in height is labeled “h.” Beneath this manometer illustration appears the label P subscript gas equal sign P subscript a t m minus sign h rho g. The third manometer has an open ended tube and is similar to the second manometer except that mercury level is higher in the right side of the tube than in the left. This difference in height is labeled “h.” Beneath this manometer illustration appears the label P subscript gas equal sign P subscript a t m plus h rho g.
Figure 12.1e A manometer can be used to measure the pressure of a gas. The (difference in) height between the liquid levels (h) is a measure of the pressure. Mercury is usually used because of its large density (credit: Chemistry (OpenStax),CC BY 4.0).

Exercise 12.1g

Check Your Learning Exercise (Text Version)

The pressure of a sample of gas is measured at sea level with an open-end mercury manometer and height (h) in open end is measured as 13.7cm below the gas height in the closed end. Assuming atmospheric pressure is 760.0 mm Hg, determine the pressure of the gas in

  1. mm Hg
  2. atm
  3. kPa

Check Your Answer[6]

Source: “Exercise 12.1g” is adapted from “8.1 Example 4” in General Chemistry 1 & 2, a derivative of Chemistry (Open Stax) by Paul Flowers, Klaus Theopold, Richard Langley & William R. Robinson, licensed under CC BY 4.0.

Example 12.1c

Calculation of Pressure Using a Closed-End Manometer

The pressure of a sample of gas is measured with a closed-end manometer, as shown to the right. The liquid in the manometer is mercury. Determine the pressure of the gas in:

  1. torr
  2. Pa
  3. bar

A diagram of a closed-end manometer is shown. To the upper left is a spherical container labeled, “gas.” This container is connected by a valve to a U-shaped tube which is labeled “closed end” at the upper right end. The container and a portion of tube that follows are shaded pink. The lower portion of the U-shaped tube is shaded grey with the height of the gray region being greater on the right side than on the left. The difference in height between the left side and right side is 26.4 c m which is indicated with horizontal line segments and arrows.

Solution

The pressure of the gas is equal to a column of mercury of height 26.4 cm. (The pressure at the bottom horizontal line is equal on both sides of the tube. The pressure on the left is due to the gas and the pressure on the right is due to 26.4 cm Hg, or mercury.) We could use the equation p = hρg as in Example 12.1b, but it is simpler to just convert between units using Table 12.1a.

  1. [latex]26.4 \;\rule[0.5ex]{2.8em}{0.1ex}\hspace{-2.8em}\text{cm Hg} \times \frac{10 \;\rule[0.25ex]{2.5em}{0.1ex}\hspace{-2.5em}\text{mm Hg}}{1 \;\rule[0.25ex]{2.5em}{0.1ex}\hspace{-2.5em}\text{mm Hg}} \times \frac{1 \;\text{torr}}{1 \;\rule[0.25ex]{2.5em}{0.1ex}\hspace{-2.5em}\text{mm Hg}} = 264 \;\text{torr}[/latex]
  2. [latex]264 \;\rule[0.5ex]{1.7em}{0.1ex}\hspace{-1.7em}\text{torr} \times \frac{1 \;\rule[0.25ex]{1.3em}{0.1ex}\hspace{-1.3em}\text{atm}}{760 \;\rule[0.25ex]{1.3em}{0.1ex}\hspace{-1.3em}\text{torr}} \times \frac{101,325 \;\text{Pa}}{1 \;\rule[0.25ex]{1.3em}{0.1ex}\hspace{-1,3em}\text{atm}} = 35,200 \;\text{Pa}[/latex]
  3. [latex]35,200 \;\rule[0.5ex]{1.2em}{0.1ex}\hspace{-1.2em}\text{Pa} \times \frac{1 \;\text{bar}}{100,000 \;\rule[0.25ex]{1em}{0.1ex}\hspace{-1em}\text{Pa}} = 0.352 \;\text{bar}[/latex]

Exercise 12.1h

The pressure of a sample of gas is measured with a closed-end manometer. The liquid in the manometer is mercury. Determine the pressure of the gas in:

  1. torr
  2. Pa
  3. bar

A diagram of a closed-end manometer is shown. To the upper left is a spherical container labeled, “gas.” This container is connected by a valve to a U-shaped tube which is labeled “closed end” at the upper right end. The container and a portion of tube that follows are shaded pink. The lower portion of the U-shaped tube is shaded grey with the height of the gray region being greater on the right side than on the left. The difference in height of 6.0 i n is indicated with horizontal line segments and arrows.

Check Your Answer[7]

Example 12.1d

Calculation of Pressure Using an Open-End Manometer

The pressure of a sample of gas is measured at sea level with an open-end Hg (mercury) manometer, as shown to the right. Determine the pressure of the gas in:

  1. mm Hg
  2. atm
  3. kPa

A diagram of an opne-end manometer is shown. To the upper left is a spherical container labeled, “gas.” This container is connected by a valve to a U-shaped tube which is labeled “open end” at the upper right end. The container and a portion of tube that follows are shaded pink. The lower portion of the U-shaped tube is shaded grey with the height of the gray region being greater on the right side than on the left. The difference in height of 13.7 c m is indicated with horizontal line segments and arrows.

Solution

The pressure of the gas equals the hydrostatic pressure due to a column of mercury of height 13.7 cm plus the pressure of the atmosphere at sea level. (The pressure at the bottom horizontal line is equal on both sides of the tube. The pressure on the left is due to the gas and the pressure on the right is due to 13.7 cm of Hg plus atmospheric pressure.)

  1. In mm Hg, this is: 137 mm Hg + 760 mm Hg = 897 mm Hg
  2. [latex]897 \;\rule[0.5ex]{3em}{0.1ex}\hspace{-3em}\text{mm Hg} \times \frac{1 \;\text{atm}}{760 \;\rule[0.25ex]{2.5em}{0.1ex}\hspace{-2.5em}\text{mm Hg}} = 1.18 \;\text{atm}[/latex]
  3. [latex]1.18 \;\rule[0.5ex]{1.8em}{0.1ex}\hspace{-1.8em}\text{atm} \times \frac{101.325 \;\text{kPa}}{1 \;\rule[0.25ex]{1.5em}{0.1ex}\hspace{-1.5em}\text{atm}} = 1.20 \times 10^2 \;\text{kPa}[/latex]

Exercise 12.1i

The pressure of a sample of gas is measured at sea level with an open-end Hg manometer, as shown to the right. Determine the pressure of the gas in:

  1. mm Hg
  2. atm
  3. kPa

A diagram of an open-end manometer is shown. To the upper left is a spherical container labeled, “gas.” This container is connected by a valve to a U-shaped tube which is labeled “open end” at the upper right end. The container and a portion of tube that follows are shaded pink. The lower portion of the U-shaped tube is shaded grey with the height of the gray region being greater on the left side than on the right. The difference in height of 4.63 i n is indicated with horizontal line segments and arrows.

Check Your Answer[8]

Measuring Blood Pressure

Blood pressure is measured using a device called a sphygmomanometer (Greek sphygmos = “pulse”). It consists of an inflatable cuff to restrict blood flow, a manometer to measure the pressure, and a method of determining when blood flow begins and when it becomes impeded (Figure 12.1f). Since its invention in 1881, it has been an essential medical device. There are many types of sphygmomanometers: manual ones that require a stethoscope and are used by medical professionals; mercury ones, used when the most accuracy is required; less accurate mechanical ones; and digital ones that can be used with little training but that have limitations. When using a sphygmomanometer, the cuff is placed around the upper arm and inflated until blood flow is completely blocked, then slowly released. As the heart beats, blood forced through the arteries causes a rise in pressure. This rise in pressure at which blood flow begins is the systolic pressure—the peak pressure in the cardiac cycle. When the cuff’s pressure equals the arterial systolic pressure, blood flows past the cuff, creating audible sounds that can be heard using a stethoscope. This is followed by a decrease in pressure as the heart’s ventricles prepare for another beat. As cuff pressure continues to decrease, eventually sound is no longer heard; this is the diastolic pressure—the lowest pressure (resting phase) in the cardiac cycle. Blood pressure units from a sphygmomanometer are in terms of millimetres of mercury (mm Hg).

A photo of a patient getting their blood pressure tested and a photo of a typical sphygmomanometer, which includes a blood pressure cuff, tubing, pump, and pressure gauge are pictured.
Figure 12.1f (a) A medical technician prepares to measure a patient’s blood pressure with a sphygmomanometer. (b) A typical sphygmomanometer uses a valved rubber bulb to inflate the cuff and a diaphragm gauge to measure pressure. (credit a: work by rawpixel.com, CC0; credit b: work by Medisave UK, CC BY 2.0)

Meteorology, Climatology, and Atmospheric Science

Throughout the ages, people have observed clouds, winds, and precipitation, trying to discern patterns and make predictions: when it is best to plant and harvest; whether it is safe to set out on a sea voyage; and much more. We now face complex weather and atmosphere-related challenges that will have a major impact on our civilization and the ecosystem. Several different scientific disciplines use chemical principles to help us better understand weather, the atmosphere, and climate. These are meteorology, climatology, and atmospheric science. Meteorology is the study of the atmosphere, atmospheric phenomena, and atmospheric effects on earth’s weather. Meteorologists seek to understand and predict the weather in the short term, which can save lives and benefit the economy. Weather forecasts are the result of thousands of measurements of air pressure, temperature, and the like, which are compiled, modelled, and analyzed in weather centres worldwide.

In terms of weather, low-pressure systems occur when the earth’s surface atmospheric pressure is lower than the surrounding environment: Moist air rises and condenses, producing clouds. Movement of moisture and air within various weather fronts instigates most weather events.

The atmosphere is the gaseous layer that surrounds a planet. Earth’s atmosphere, which is roughly 100–125 km thick, consists of roughly 78.1% nitrogen and 21.0% oxygen, and can be subdivided further into the regions shown in Figure 12.1h: the exosphere (furthest from earth, > 700 km above sea level), the thermosphere (80–700 km), the mesosphere (50–80 km), the stratosphere (second lowest level of our atmosphere, 12–50 km above sea level), and the troposphere (up to 12 km above sea level, roughly 80% of the earth’s atmosphere by mass and the layer where most weather events originate). As you go higher in the troposphere, air density and temperature both decrease.

This diagram shows half of a two dimensional view of the earth in blue and green. A narrow white layer, labeled “troposphere 0 dash 12 k m” covers this hemisphere. This layer is also labeled “layer where most weather events originate.” Next, a thicker light blue layer labeled “Stratosphere 12 dash 50 k m” is shown. This is followed by a slightly thinner layer also in light blue labeled “Mesosphere 50 dash 80 k m.” Following this layer is a relatively thick light blue layer labeled “Thermosphere 80 dash 700 k m.” A blue layer appears that covers the rightmost two thirds of the diagram. This region gradually darkens from a lighter blue at the left to a dark blue at the right. This region of the diagram is labeled “exosphere greater than 700 k m.”
Figure 12.1g Earth’s atmosphere has five layers: the troposphere, the stratosphere, the mesosphere, the thermosphere, and the exosphere.

Climatology is the study of the climate, averaged weather conditions over long time periods, using atmospheric data. However, climatologists study patterns and effects that occur over decades, centuries, and millennia, rather than shorter time frames of hours, days, and weeks like meteorologists. Atmospheric science is an even broader field, combining meteorology, climatology, and other scientific disciplines that study the atmosphere (credit: Chemistry (OpenStax),CC BY 4.0).

Links to Interactive Learning Tools

Explore Pressure Concepts from the Physics Classroom.

Key Equations

  • [latex]P = \frac{F}{A}[/latex]
  • [latex]p = h \rho g[/latex]

Attribution & References

Except where otherwise noted, this page is adapted by JR van Haarlem from “8.1 Gas Pressure” In General Chemistry 1 & 2 by Rice University, a derivative of Chemistry (Open Stax) by Paul Flowers, Klaus Theopold, Richard Langley & William R. Robinson and is licensed under CC BY 4.0. ​Access for free at Chemistry (OpenStax)​
  1. 2.2 x 102 kPa ↵
  2. 0.974 atm; 740 mm Hg; 98.7 kPa; 0.987 bar ↵
  3. Lying down distributes your weight over a larger surface area, exerting less pressure on the ice compared to standing up. If you exert less pressure, you are less likely to break through thin ice. ↵
  4. 10.3 m ↵
  5. 0.809 atm and 82.0 kPa ↵
  6. (a) 623 mm Hg; (b) 0.820 atm; (c) 83.1 kPa ↵
  7. (a) ~150 torr; (b) ~20,000 Pa; (c) ~0.20 bar ↵
  8. (a) 642 mm Hg; (b) 0.845 atm; (c) 85.6 kPa ↵
definition

License

Icon for the Creative Commons Attribution 4.0 International License

Chemistry v. 1 backup Copyright © 2023 by Gregory Anderson; Caryn Fahey; Jackie MacDonald; Adrienne Richards; Samantha Sullivan Sauer; J.R. van Haarlem; and David Wegman is licensed under a Creative Commons Attribution 4.0 International License, except where otherwise noted.

Share This Book