CHEM 1001/CHM 1020/ Chm1025C/CHM1032C         Name:_Answers

Module 6 SamplePretest   

Module Six: The Gaseous State  (Chapter 11)

A1. ____(12) Properties of Solids, Liquids, and Gaes

A._____(10) Kinetic Molecular Theory-Section 11.10  Answer

B._____(00) Bonus: Discussion Real vs Ideal Gas Equation-Sect 11.10

C._____(05) Standard Conditions/Molar Volume-Sect 9.5

D._____(10) Gas Laws/Vocabulary-Sections 11.4, 11.5, 11.6, 11.7, 11.8, 11.9

E._____(20) Gas Law Problems- Sections 11.4, 11.5, 11.6, 11.7, 11.8, 11.9

F. ____ (10) Volume-Volume Stoichiometry Problem-Section 10.6

G._____(10) Mass-Volume Stoichiometry Problem-Section 10.5

M._____(25) Multiple Choice Application Chapter 11


______(102) Total = ______%


Module Six- Part A: Kinetic Molecular Theory ANSWERS  10 points


 State the assumptions of the Kinetic Molecular theory as stated in the book pages 299-300:


1. Gases are composed of molecules*[1].  The distance between the molecules is very-very great compared to the size of the molecules themselves, and the total volume of the molecules is only a very-very small fraction of the entire space occupied by the gas.  Therefore, considering volume, we are primary considering empty space.  (This assumption explains why gases are highly compressed and have very low densities.)


(Gases are made up of very tiny molecules. The volume of a gas is mainly empty space).

2. No attractive forces exist between molecules in a gas.  (This is what keeps a gas from spontaneously becoming a liquid.)

(Gas molecules have no attraction for one another.)


3. The molecules of a gas are in a state of constant, rapid motion, colliding with each other and with the walls of the container in a perfectly random manner.  (This assumption explains why different gases normally mix completely.  The collisions between molecules and the walls of the container account for the pressure exerted by the gas.)

(Gas molecules demonstrate rapid motion, move in straight lines, and travel in random directions.)

4. All of these molecular collisions are perfectly elastic. As a result, the system as a whole experiences no loss of kinetic energy, the energy derived from the motion of a particle.

(Gas molecules undergo perfect elastic collisions.)


5. The average kinetic energy per molecule of a gas is proportional to the absolute temperature, and the average kinetic energy per molecule is the same at a given temperature and pressure for all gases. 

(The average kinetic energy of gas molecules is proportional to the Kelvin temperature, that is KE is approximately T.)


For shorter answers reference section 11.10 page 299-300 and write only the bold black sentences. Or see the bold red above.

[1]When we think of molecules of elemental gases, we usually think of the diatomic gases such as nitrogen, oxygen, hydrogen, etc. The Nobel gases exist as monoatomic gases such as Helium, Neon, etc.