7. Gases

Pressure Units

Pressure Units and Pressure Unit Conversion Explained

Atmospheric pressure at the top of Pikes Peak in Colorado is approximately 480 mm Hg. Convert this value to atmospheres and to pascals.

Hurricane Wilma of 2005 is the most intense hurricane on 
record in the Atlantic basin, with a low-pressure reading of 
882 mbar (millibars). Convert this reading into (c) inches of Hg.

The pressure on top of Mount Everest (29,029 ft) averages about
235 mmHg. Convert this pressure to each indicated unit.
a. torr
b. psi
c. in Hg
d. atm

Conversion of Pressure Units in Chemistry

Pakistan’s K2 is the world’s second-tallest mountain, with an altitude of 28,251 ft. Its base camp, where climbers stop to acclimate, is located about 16,400 ft above sea level.
(a) Approximate atmospheric pressure P at different altitudes is given by the equation P = e-h>7000, where P is in atmospheres and h is the altitude in meters. What is the approximate atmospheric pressure in mm Hg at K2 base camp?

A glass tube has one end in a dish of mercury and the other
end closed by a stopcock. The distance from the surface of
the mercury to the bottom of the stopcock is 850 mm. The
apparatus is at 25 °C, and the mercury level in the tube is
the same as that in the dish.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/6142d25a3dd7bf23-1669647327315.jpg" alt="" />
(a) Show on drawing (1) what the approximate level of
mercury in the tube will be when the temperature of the
entire apparatus is lowered from +25 °C to -25 °C.

Assume that you have an open-end manometer filled with ethyl
alcohol 1density = 0.7893 g>mL at 20 °C2 rather than mercury
1density = 13.546 g>mL at 20 °C2. What is the pressure
in pascals if the level in the arm open to the atmosphere is
55.1 cm higher than the level in the arm connected to the gas
sample and the atmospheric pressure reading is 752.3 mm Hg?

Pressure Units Example 1

The recommended pressure for inflation of an automobile 
tire is 35 psi. What is the pressure in units of mm Hg? 
11 atm = 14.7 psi; 1 atm = 760 mm Hg2 (LO 10.1) 
(a) 3.9 * 105 mm Hg 
(b) 0.68 mm Hg 
(c) 3.2 * 102 mm Hg 
(d) 1.8 * 103 mm Hg

Hurricane Wilma of 2005 is the most intense hurricane on 
record in the Atlantic basin, with a low-pressure reading of 
882 mbar (millibars). Convert this reading into (b) torr.

Given a barometric pressure of 751.5 mmHg, calculate the pressure
of each gas sample as indicated by the manometer.
(a) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/21bb646d8be21c22-1659976454301.jpg" alt="" />

The different units for Pressure

The pressure in Denver, Colorado (elevation 5280 ft), averages
about 24.9 in Hg. Convert this pressure to each indicated unit.
a. atm

Carry out the following conversions:
(a) 352 torr to kPa

A person weighing 75 kg is standing on a threelegged
stool. The stool momentarily tilts so that the entire
weight is on one foot. If the contact area of each foot
is 5.0 cm2, calculate the pressure exerted on the underlying
surface in (a) bars

Gas Pressure and Converting Units of Pressure

(a) The compound 1-iodododecane is a nonvolatile liquid
with a density of 1.20 g>mL. The density of mercury is
13.6 g>mL. What do you predict for the height of a barometer
column based on 1-iodododecane, when the atmospheric
pressure is 749 torr?

Hurricane Wilma of 2005 is the most intense hurricane on
record in the Atlantic basin, with a low-pressure reading of
882 mbar (millibars). Convert this reading into (a) atmospheres.

Given a barometric pressure of 751.5 mmHg, calculate the pressure
of each gas sample as indicated by the manometer.
(b)

The North American record for highest recorded barometric
pressure is 31.85 in Hg, set in 1989 in Northway, Alaska. Convert
this pressure to each indicated unit.
a. mmHg

The pressure in Denver, Colorado (elevation 5280 ft), averages
about 24.9 in Hg. Convert this pressure to each indicated unit.
c. psi

Name the regions of the atmosphere. What property is used 
to distinguish between different regions of the atmosphere?

(b) What pressure, in atmospheres, is exerted
on the body of a diver if she is 10 m below the surface of the
water when the atmospheric pressure is 100 kPa? 
Assume that the density of the water is 1.00 5 1.00 3 103 kg/m3. The
gravitational constant is 9.81 m/s2, and 1 Pa 5 1 kg/ms2

The pressure in Denver, Colorado (elevation 5280 ft), averages
about 24.9 in Hg. Convert this pressure to each indicated unit.
b. mmHg

An ordinary gasoline can measuring 30.0 cm by 20.0 cm by
15.0 cm is evacuated with a vacuum pump. Assuming that virtually
all of the air can be removed from inside the can and that
atmospheric pressure is 14.7 psi, what is the total force (in
pounds) on the surface of the can? Do you think that the can
could withstand the force?

If the atmospheric pressure is 0.995 atm, what is the pressure
of the enclosed gas in each of the three cases depicted in the
drawing? Assume that the gray liquid is mercury.
(ii) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/95eec773cdff9207-1676479771038.jpg" alt="" />

A person weighing 75 kg is standing on a threelegged
stool. The stool momentarily tilts so that the entire
weight is on one foot. If the contact area of each foot
is 5.0 cm2, calculate the pressure exerted on the underlying
surface in (c) pounds per square inch

(b) Which units are appropriate
for expressing atmospheric pressures, N, Pa, atm, kg>m2?

An open-end manometer containing mercury is connected
to a container of gas, as depicted in Sample Exercise 10.2.
What is the pressure of the enclosed gas in torr in each of the
following situations? (a) The mercury in the arm attached
to the gas is 15.4 mm higher than in the one open to the atmosphere;
atmospheric pressure is 0.985 atm.

The troposphere contains about three quarters of the mass 
of the entire atmosphere. The troposphere is only 12 km 
thick while the whole atmosphere is about 120 km thick. 
Explain why the troposphere contains such a large fraction 
of the total mass.

The pressure in Denver, Colorado (elevation 5280 ft), averages 
about 24.9 in Hg. Convert this pressure to each indicated unit. 
d. Pa

Pressure&nbsp;represents the force that a gas molecule exerts against the walls of its container. It can be depicted as force per area.

If the atmospheric pressure is 0.995 atm, what is the pressure
of the enclosed gas in each of the three cases depicted in the
drawing? Assume that the gray liquid is mercury.
(i) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/59c5da5ca7b9e5e2-1660662110150.jpg" alt="" />

Perform the following conversions: (d) 1.323 * 105 Pa to atmospheres

Carry out the following conversions: 
(b) 0.255 atm to mm Hg

Pressure Units Defined

The highest barometric pressure ever recorded was 823.7 torr at Agata in Siberia, Russia on December 31, 1968. Convert this pressure to (c) pascals.

Yet another common measure of pressure is the unit pounds 
per square inch (psi). How many pounds per square inch 
correspond to 1.00 atm? To 1.00 mm Hg?

Pressure and Pressure Units

The highest barometric pressure ever recorded was 823.7 torr at Agata in Siberia, Russia on December 31, 1968. Convert this pressure to (e) psi.

What is the pressure in millimeters of mercury inside a container 
of gas connected to a mercury-filled open-end manometer 
of the sort shown in Figure 10.5 when the level in 
the arm connected to the container is 17.6 cm lower than the 
level in the arm open to the atmosphere and the atmospheric 
pressure reading outside the apparatus is 754.3 mm Hg?

What is the pressure in atmospheres inside a container of gas 
connected to a mercury-filled open-end manometer when the 
level in the arm connected to the container is 28.3 cm higher 
than the level in the arm open to the atmosphere and the atmospheric 
pressure reading outside the apparatus is 1.021 atm?

The highest barometric pressure ever recorded was 823.7 torr at Agata in Siberia, Russia on December 31, 1968. Convert this pressure to (d) bars.

(a) How are the boundaries between the regions of the atmosphere determined?

(a) How high in meters must a column of ethanol be to exert
a pressure equal to that of a 100-mm column of mercury?
The density of ethanol is 0.79 g/mL, whereas that of mercury
is 13.6 g/mL. 
Assume that the density of the water is 1.00 5 1.00 3 103 kg/m3. The
gravitational constant is 9.81 m/s2, and 1 Pa 5 1 kg/ms2.

Pressure Units Example 2

What is the pressure of the gas inside the bulb (atm) if the 
outside pressure is 0.92 atm?

(a) 1.1 atm (b) 2.6 atm 
(c) 0.22 atm (d) 0.70 atm

(d) If you measure pressure in bars instead 
of atmospheres, calculate the corresponding value of 
R in L-bar/mol-K.

If the density of water is 1.00 g/mL and the density of mercury is 13.6 g/mL, how high a column of water in meters can be supported by standard atmospheric pressure? By 1 bar?

The world record for lowest pressure (at sea level) was 
652.5 mmHg recorded inside Typhoon Tip on October 12, 1979, 
in the western Pacific Ocean. Convert this pressure to each 
indicated unit. 
b. atm

The world record for lowest pressure (at sea level) was 
652.5 mmHg recorded inside Typhoon Tip on October 12, 1979, 
in the western Pacific Ocean. Convert this pressure to each 
indicated unit. 
d. psi

Units of Pressure

Perform the following conversions: (b) 0.685 bar to kilopascals

(b) Explain why the stratosphere, which is about 35 km thick, has a smaller total mass than the troposphere, which is about 12 km thick.

What is Pressure? | Physics | Don't Memorise

Torricelli, who invented the barometer, used mercury in
its construction because mercury has a very high density,
which makes it possible to make a more compact barometer
than one based on a less dense fluid. Calculate the density
of mercury using the observation that the column of
mercury is 760 mm high when the atmospheric pressure is
1.01 * 105 Pa. Assume the tube containing the mercury is
a cylinder with a constant cross-sectional area.

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[BOOK CHEM] Clutch Version

Partial Pressure

Partial Pressure (PGas) is the pressure exerted by an individual gas within a container.

Velocity Distributions

Velocity Distributions represent probability distributions for a gas when examining their molar mass and temperature.

Mole Fraction

Mole Fraction (X) represents the mole component by total moles.&nbsp;

Mole Fraction -

The Ideal Gas Law Derivations

The&nbsp;Ideal Gas Law Derivations are a convenient way to solve gas calculations involving 2 sets of the same variables.&nbsp;

Root Mean Square Speed

Root Mean Square Speed&nbsp;allows for the determination of the velocity of 1 type of gas molecule.

The Ideal Gas Law: Density

Under certain conditions of pressure and temperature, the Ideal Gas Law can determine the density&nbsp;of a gas.&nbsp;

Effusion

Effusion is the escaping of gas molecules or atoms through a pinhole.&nbsp;

Kinetic Energy of Gases

Kinetic Energy is the energy an object possesses due to its motion.

Gas Stoichiometry

Gas Stoichiometry involves chemical reactions that contain gases.

The Ideal Gas Law

The Ideal Gas Law formula relates the behavior of gases under varying conditions of pressure, volume, moles and temperature.

Chemistry Gas Laws: Combined Gas Law

The Combined Gas Law&nbsp;is created from “combining” Boyle’s Law, Charles’ Law, and Gay–Lussac’s Law.

Pressure is the force that is exerted within a given volume of space.&nbsp;

Kinetic Molecular Theory

A gas is seen as a collection of molecules or individual atoms that are in constant motion. The Kinetic-Molecular Theory tries to use data of real gases to predict how an ideal gas would behave if they existed.&nbsp;&nbsp;

Standard Temperature and Pressure

In order to accurately study the effect that changes in pressure, temperature and moles have on volume, chemists will often run their experiments under Standard Temperature and Pressure.&nbsp;

The Ideal Gas Law Applications

The Ideal Gas Law Applications establish both the direct and inverse relationships between the Ideal Gas Law variables.

Maxwell-Boltzmann Distribution

The Maxwell-Boltzmann Distribution is a probability distribution curve that describes the speed of a gas at a specific temperature.

Chemistry Gas Laws

Chemistry Gas Laws&nbsp;are laws that relate together the pressure, volume and temperature of a gas.

The Ideal Gas Law: Molar Mass

The Ideal Gas Law can be further extended to find the molar mass of a gas.&nbsp;

Van der Waals Equation

The&nbsp;Van der Waals Equation is used when dealing with real, non-ideal gases.&nbsp;