Name ______________________ # ________
Honors Chemistry
Carpenito/Dinota
Reading Guide: Gases
(blue book – Ch.13 yellow book – Ch.5)
Section: Units of Pressure & Measurement (blue 13.1, yellow 5.1)
Define the terms:
pressure:
barometer:
manometer:
What is standard atmospheric pressure in the following units?
__________ atm __________ mm Hg __________ torr ___________ kPa __________ in Hg __________ psi
Describe a simple mercury barometer. How is this barometer used to measure the pressure of the atmosphere? How
would the atmospheric pressure atop Mt. Everest compare when measured on this barometer? Why?
When measuring the pressure of a gas in a container with a manometer…
If the pressure of the atmosphere is greater than the pressure of the contained gas, then how do you calculate
the pressure of the gas?
If the pressure of the atmosphere is less than the pressure of the contained gas, then how do you calculate the
pressure of the contained gas?
Convert the following pressures:
a. 105.2 kPa =
__________ atm
b. 752 mmHg =
__________ kPa
c. 774 torr =
__________ atm
d. 28.5 in Hg =
__________ atm
Section: Relationships Between Pressure, Volume, & Temperature (blue 13.2, 13.3, yellow 5.2)
Define the terms:
Boyles law:
Charles’s law:
Gay-Lussac’s law:
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combined gas law:
In ANY calculation involving the behavior of gases, which unit of temperature is necessary?
Draw and identify the relationships between the following sets of variables:
Boyle’s Law
P
Charles’s Law
V
Gay-Lussac’s Law
P
V
T
T
Type of relationship
Type of relationship
Type of relationship
____________________
____________________
____________________
The pressure in a car tire is 198 kPa at 27C. After a long drive, the pressure is 225 kPa. What is the temperature of the
air in the tire? Assume that the volume of the tire is constant.
A balloon inflated in a room at 20C has a volume of 5.00 L. The balloon is then heated to a temperature of 62C. What
is the new volume if the pressure remains constant?
Nitrous oxide (N2O) is used as an anesthetic. The pressure on 2.50 L of N2O changes from 105 kPa to 40.5 kPa. If the
temperature does not change, what will the new volume be?
A 5.00 L air sample has a pressure of 107 kPa at a temperature of -50C. If the temperature is raised to 102C and the
volume expands to 7.00 L, what will the new pressure be?
Section: Ideal Gas Law (blue 13.5, yellow 5.2, 5.3)
Define the terms:
ideal gas law:
universal gas constant:
What can the ideal gas law calculate that the combined gas law can not?
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What pressure is exerted by 0.450 mol of a gas at 25C if the gas is in a 0.650 L container?
A child’s lungs can hold 2.20 L of air. How many grams of air do her lungs hold at a pressure of 102 kPa and a body
temperature of 37C? (use molar mass of 29 g for air)
Another equation may be derived from the ideal gas law in order to calculate the density of a gas. What is this
equation? (Remember: n = grams/molar mass and d = g/L)
What is the density of butane, C4H10, (in grams per liter) at 97C and 755 mm Hg?
Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and 25C, it has a
density of 1.71 g/L. What is the molar mass of cyclopropane?
Section : Avogadro’s Law (blue 13.4, yellow 5.2)
Define the terms:
Avogadro’s law:
What is the relationship between the volume of a gas and the number of moles of the gas?
If 0.214 mol of argon gas occupies a volume of 652 mL at a particular temperature and pressure, what volume would
0.375 mol of argon occupy under the same conditions?
Section : Dalton’s Law of Partial Pressures (blue 13.6, yellow 5.5)
Define the terms:
partial pressure:
Dalton’s law of partial pressure:
A mixture of three gases N2, O2 , and CO2 are contained in a system at STP. The partial pressure of N2 is 30.6 kPa and the
partial pressure of O2 is 25.9 kPa. What is the partial pressure of CO2?
A 2.5 L flask contains a mixture f nitrogen gas and oxygen gas at 25C . The total pressure of the gaseous mixture is 0.95
atm, and the mixture is known to contain 0.040 mol N2. Calculate the partial pressure of oxygen and the moles of
oxygen present.
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Section : Graham’s Law (yellow 5.6)
Define the terms:
effusion:
Graham’s law:
Which two factors affect the relative rates of effusion of different gases?
How do the rates of effusion of gases with large molar masses differ from those of gases with small molar masses?
Rank the following gases in order of increasing speed of effusion through a tiny opening.
NO
Ar
N2
N2O5
A gas effuses 1.55 times faster than propane (C3H8) at the same temperature and pressure. Is the gas heavier or lighter
than propane? What is the molar mass of the gas?
A balloon filled with nitrogen gas has a small leak. Another balloon filled with hydrogen gas has an identical leak. How
much faster will the hydrogen balloon deflate?
Section : Ideal Gases vs. Real Gases (blue 13.8, 13.10, yellow 5.7)
Define the terms:
kinetic molecular theory:
ideal gas:
real gas:
Under what conditions do real gases behave most like ideal gases?
Use the kinetic theory of gases to explain the statement, “No gas exhibits ideal behavior at all temperatures and
pressures.”
What real gas comes closest to having the characteristics of an ideal gas? Explain your answer.
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