Must be own work and use in text citation and references. (Part 1): Answer discussion question below 2 full paragraph (4-5 sentences EACH paragraph. 1. What is the ideal gas law? What factors cause gases to deviate from ideal behavior? Give specific examples. (Part 2): Reply to ALL 3 of the below post, each must be 1 full paragraph (4-5 sentences). THERE SHOULD BE A TOTAL OF 3 PARAGRAPHS. 1. The ideal gas law can be explained by the kinetic molecular theory. We define ideal gas as consisting of molecules with negligible volume that are in constant random. The ideal gas law states the relationship between absolute pressure (P), volume (V), and absolute temperature (T) in a theoretical, "ideal" gas. Mathematically, the ideal gas law is: PV = nRT, where P is absolute pressure, V is volume, n is the number of moles of a gas, R is the universal gas constant, and T is temperature. Real gases deviate from the ideal gas law at high pressure and low temperature following kinetic theory postulates 1 and 3. From kinetic theory, we expect these deviations, because real molecules do have volume and intermolecular forces do exist. An example of an ideal gas law could be a hot air balloon. As the gas in the hot air balloon is heated (by fire), the volume of the hot air balloon will increase which allows it to fly. 2. The ideal gas law is the equation PV= nRT, which combines all of the gas laws. The variables being: (P) pressure; (V) volume; (n) number of mole of gas; and (T) temperature, leaving the constant (R) gas constant. The ideal gas law includes all the information contained in Boyle's, Charles"s and Avogardo's laws. And the ideal gas law is most accurate for low to moderate pressures and for temps that are not too low. Volume, temperature and pressure can cause a deviation in the law. 3. The ideal gas law comes from the kinetic theory, and summarizes how a gas reacts under different conditions, such as temperature, volume and pressure. To find the ideal gas law from the kinetic theory, you must first find the pressure by multiplying frequency of collisions by the average force. To find the average force you must know its mass as well as its average speed or momentum. In other words, the larger and faster the molecule, the more it will be shown in the force. The finished equation should be PV=nRT. In order for a gas to be an ideal gas, it must first follow the 5 postulates of the Kinetic Theory. Some factors that would cause non ideal behavior would be increased pressure, causing intermolecular forces to increase within molecules. UMT University of Management and Technology MGT 150. Project Management Course Assignments Assignment 1 • Bottom-up cost estimating exercise (Module 3, pp 19-20) • Parametric cost estimate exercise (Module 3, pp. 43-44) • For the table below o Create a PERT/CPM chart o Compute project duration o Compute Latest Start, Earliest Start, and Float (Slack) Task Predecessor Duration (in.

1. Must be own work and use in text citation and references.
(Part 1): Answer discussion question below 2 full paragraph (4-
5 sentences EACH paragraph.
1. What is the ideal gas law? What factors cause gases to
deviate from ideal behavior? Give specific examples.
(Part 2): Reply to ALL 3 of the below post, each must be 1 full
paragraph (4-5 sentences). THERE SHOULD BE A TOTAL OF
3 PARAGRAPHS.
1. The ideal gas law can be explained by the kinetic molecular
theory. We define ideal gas as consisting of molecules with
negligible volume that are in constant random. The ideal gas
law states the relationship between absolute pressure (P),
volume (V), and absolute temperature (T) in a theoretical,
"ideal" gas. Mathematically, the ideal gas law is: PV = nRT,
where P is absolute pressure, V is volume, n is the number of
moles of a gas, R is the universal gas constant, and T is
temperature. Real gases deviate from the ideal gas law at high
pressure and low temperature following kinetic theory
postulates 1 and 3. From kinetic theory, we expect these
deviations, because real molecules do have volume and
intermolecular forces do exist. An example of an ideal gas law
could be a hot air balloon. As the gas in the hot air balloon is
heated (by fire), the volume of the hot air balloon will increase
which allows it to fly.
2. The ideal gas law is the equation PV= nRT, which combines
all of the gas laws. The variables being: (P) pressure; (V)
volume; (n) number of mole of gas; and (T) temperature,
leaving the constant (R) gas constant. The ideal gas law
includes all the information contained in Boyle's, Charles"s and
Avogardo's laws. And the ideal gas law is most accurate for low
to moderate pressures and for temps that are not too low.
Volume, temperature and pressure can cause a deviation in the

2. law.
3. The ideal gas law comes from the kinetic theory, and
summarizes how a gas reacts under different conditions, such as
temperature, volume and pressure. To find the ideal gas law
from the kinetic theory, you must first find the pressure by
multiplying frequency of collisions by the average force. To
find the average force you must know its mass as well as its
average speed or momentum. In other words, the larger and
faster the molecule, the more it will be shown in the force. The
finished equation should be PV=nRT. In order for a gas to be an
ideal gas, it must first follow the 5 postulates of the Kinetic
Theory. Some factors that would cause non ideal behavior
would be increased pressure, causing intermolecular forces to
increase within molecules.
UMT
University of Management and Technology
MGT 150. Project Management
Course Assignments
Assignment 1
• Bottom-up cost estimating exercise (Module 3, pp 19-20)
• Parametric cost estimate exercise (Module 3, pp. 43-44)

3. • For the table below
o Create a PERT/CPM chart
o Compute project duration
o Compute Latest Start, Earliest Start, and Float (Slack)
Task Predecessor Duration (in days)
Latest
start
Earliest
start
Float
(slack)
A Start 6
B A,D 8
C B 10
D Start 7
E D 12
F Start 12
G F 12
• Exercise 3-2 (Module 3, p. 61)
• Exercise 3-3 (Module 3, pp. 63-64)
UMT 2

4. -2008 University of Management and Technology
MGT150
Assignment 2
Following are cost and schedule data for a project that is
underway.
Month 1 2 3 4 5 6 7 8 9 10 11 12
Planned 30 35 42 46 40 52 45 48 50 40 30 15
Actual 10 25 47 55 52 54 50 58
Project Cost Data
Task Planned start Planned
Duration
Actual start Actual
Duration
A Beginning
Month 1
2 months Beginning
Month 2
2.5 months
B Beginning
Month 2
3 months Beginning
Month 3

5. 4 months
C Beginning
Month 4
3 months Beginning
Month 5
3.5 months
D Beginning
Month 6
5 months Beginning
Month 7
2 months so far
E Beginning
Month 8
4 months Not yet
begun
F Beginning
Month 10
3 months Not yet
begun
Project Schedule Data

6. 1. Using the cost data in the cost table above, create a
cumulative cost curve
comparing actual versus planned costs (Note: with the
cumulative cost curve
– also called the S-curve – you must cumulate the cost data. See
More Info,
Module 3, p. 53.)
2. Using the schedule data in the schedule table above, create a
Gantt chart
comparing actual versus planned schedule performance
3. Summarize in words what you see project status to be at this
time. What do
you predict regarding the final cost and final schedule for the
project? Note,
by looking at the schedule and cost day simultaneously, you are
engaging in
integrated cost/schedule control.
UMT 3
-2008 University of Management and Technology
MGT150
Assignment 3
Following are data reporting progress on a project. Work on all

7. tasks contained in
the table is scheduled to be complete as of the day of the report.
Budget Begun? Complete? Actual
cost
Earned
Value
Sched
var
Cost
var
Task A 300 Yes Yes 325
Task B 400 Yes Yes 450
Task C 250 Yes Yes 225
Task D 425 Yes No 250
Task E 350 Yes Yes 400
Task F 250 No No 0
TOTAL
Questions
1. Using the 50-50 Rule, what is earned value for this project?
(Put answer into the
“Earned value” column in the table.)
2. Using the 0-100 Rule, what is earned value for this project?
(Simply supply the
number)
3. Note the discrepancy of earned value figures when using the

8. 50-50 Rule and 0-
100 Rule. Why is there a discrepancy? Which Rule should we
use? Explain your
rationale.
4. Using the 50-50 Rule earned value computation, what is
schedule variance for
the project as reported? (Put answer into the “Sched var”
column in the table.)
5. What is the schedule performance index (SPI)? (Provide the
number. What does
this number mean?)
6. Using the 50-50 Rule earned value computation, what is the
cost variance for
the project as reported? (Put answer into the “Cost var” column
in the table.)
7. What is the cost performance index (CPI)? (Provide the
number. What does this
number mean?)
8. If the total budget for this project is 5000, use CPI to
compute estimate at
complete (EAC).
9. Using the earned value information garnered from the above
table, provide your
boss a brief status report on project progress to date. Also,
provide projections
for future status.
Must be own work and use in text citation and references.

9. (Part 1): Answer discussion question below 2 full paragraph (4-
5 sentences EACH paragraph.
1. Please discuss the Kinetic Theory giving all of the postulates.
What role does temperature play? What causes pressure
according to this theory? What are some of the problems with
this theory?
(Part 2): Reply to ALL 3 of the below post, each must be 1 full
paragraph (4-5 sentences). THERE SHOULD BE A TOTAL OF
3 PARAGRAPHS.
1. The Kinetic theory leads to the gas law. However, the “gas
consist of molecules in constant random motion” (Ebbing &
Gammon, 2012, p. 162). There are five postulates in the kinetic
theory. Postulate 1 states that gases are composed of molecules
whose size is negligible compared with the average distance
between them, postulate 2 states that molecules move randomly
in straight lines in all directions and at various speeds, postulate
3 states the forces of attraction or repulsion between two
molecules in a gas are very weak or negligible, except when
they collide, postulate 4 states when molecules collide with one
another, the collisions are elastic, and lastly, postulate 5 states
that the average kinetic energy of a molecule is proportional to
the absolute temperature (Ebbing & Gammon, 2012, p.163). On
the other hand, the temperature plays a role in the degree of
freedom. However, when the kinetic energy per degree of
freedom, the constant proportionality of the temperature is ½
times Boltzmann constant. Another word, the temperature will
decrease when the pressure drops to a certain point, then this
result will relate to the equipartition theorem. As for what will
cause the pressure in this theory is due to the force and
frequency of molecular collisions within the container walls.
One major problem that was determined with the kinetic theory
was the equation of spatial distribution of temperature and heat.
2. According to our text on pgs 162 - 164, the kinetic theory
states that a gas consists of molecules in constant random
motion. The 5 postulates that relate to this theory are: 1. Gases

10. are composed of molecules whose size is negligible compared
with the average distance between them. 2. Molecules move
randomly in straight lines in all directions and at various
speeds. 3. The forces of attraction or repulsion between two
molecules in a gas are very weak or negligible, except when
they collide. 4. When molecules collide with one another, the
collisions are elastic; and 5. The average kinetic energy of a
molecule is proportional to the absolute
temperature.Temperature plays a role in that the higher the
temperature, the greater the molecular kinetic energy. Pressure
is caused due to the force and frequency of molecular collisions
with the container wall. If you increase the number of gas
molecules within a container; while not increasing the container
size, the frequency of collisions of the gas molecules with the
walls of the container will increase causing the pressure to
increase. Once the container size is adjusted (increased) this
will lessen the frequency of collisions with the container walls
and lessen the pressure within the container.
3. Kinetic Theory is the body of theory that explains the
physical properties of matter in terms of the motions of its
constituent particles. Temperature plays a role in Kinetic theory
when molecules are rapidly moving causing friction which
causesheat. It also states that the gas pressure is due to the
impacts of the molecules moving fast