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.