Leader:Lea
Course:Chem 177
Instructor:Dr. Schewe-Miller
Date:4/16/2013
Equations:
PV=nRT
P1V1 = P2V2
V1/T1 = V2/T2
V1/N1 = V2/N2
n/V = P/RT
d = PM/RT
M = dRT/P
Worksheet 4.2 - Ideal Gas Law
Supplemental Instruction
Iowa State University
Gas Law Constants:
.08206 L*atm/mol*K
8.314 J/mol*K
1.987 cal/mol*K
8.314 (m^3)Pa/mol*K
62.36 L*torr/mol*K
1. Will one mole of argon atoms at a given temperature and pressure have the same volume as a
mole of xenon atoms at the same temperature and pressure? Will they have the same
densities? Why or why not?
2. Calculate the number of molecules of air inhaled, assuming the volume of the inhalation is
2.25 L at body temperature, 37 °C, with a pressure of 735 torr.
3. For the following laws, state whether the relationship between the two variables listed is
directly proportional or inversely proportional.
a. Boyles law: pressure and volume
b. Charles law: volume and temperature
c. Avogadro’s law: volume and number of molecules
4. A sample containing two moles of hydrogen molecules, kept at 25 degrees C and 1
atmosphere of pressure, is originally 44.8 liters. What will the volume be if the temperature of
the sample is increased to 30 degrees C?
5. Calculate the molar mass of a gas if 2.50 g occupies 0.875 L at 3 atm and 33 °C.
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6. Calculate the density of a hypothetical gas if 3 moles occupy 1.2L at 760 torr and 25 degrees
C