Module 6 DBA & Exam Review 
Edited question 30 on 02/02/23 

This review is neither a replica of the exam nor does it contain every concept in the module.  It is always best practice to review all lessons and assessments and ensure you have the completed journals. Resubmitting is a great way to review/learn and improve your grade.   In this review, questions 1 – 24 are the general topics for the multiple choice type questions on the module exam; questions 25-26 are covered as an essay on the exam. Questions 27 - 31 are the honors extension questions. Be sure that any reaction given is balanced on the exam prior to completing stoichiometry. The number in parenthesis is the corresponding lesson. Please reach out to your instructor with any questions (Answer key)
Segment 2 Formula Sheet - Google Copy
Segment 2 Formula Sheet - RTF download

●	Module 6 Regular Exam: There are 17 questions on the actual exam
○	16 multiple choice and 1 essay/free response.
●	Module 6 Honors Exam: There are 21 questions on the actual exam
○	19 multiple choice and 2 essay/free responses.

Multiple Choice format questions:
1.	Define and give an example of converting potential energy to kinetic energy.  (6.01) 

2.	Define and give an example of converting radiant (light) energy to chemical energy. (6.01)  

3.	Compare stored mechanical energy and mechanical energy. (6.01) 

4.	What is the average kinetic energy of a substance? What unit do we use? (6.01)

5.	Relate temperature and molecular motion. (6.01) 

6.	Explain the kinetic molecular theory and list the postulates. (6.02)  

7.	Identify the characteristics of a solid, liquid, gas and plasma. (6.02) 

8.	Identify a substance that expands to fill the container it is in.(6.02)  

9.	What state of matter has the kinetic energy of its particles high enough to completely overcome the intermolecular forces of attraction between them?  (6.02)

10.	How does the arrangement of the particles in a solid compare to that of a liquid and a gas? (6.02) 

11.	Explain how kinetic energy compares in a solid, liquid and a gas. (6.01/6.02) 

12.	What happens to a substance as the kinetic energy increases? (6.01/6.02)  

13.	What happens to a substance as the kinetic energy decreases? (6.03) 

14.	A list of changes is shown. (6.01/6.02)
a.	Molecules move more random
b.	Collisions are more elastic
c.	Boiling
d.	Intermolecular bonds become stronger
e.	Evaporation
f.	Condensation
g.	Loses energy
h.	Molecules vibrate faster

Which of the above changes would be accompanied by a decrease of temperature?

15.	Using the diagram to the right, what is the approximate freezing point, melting point and boiling point? (6.03)

16.	Using the diagram to the right, what is the state of matter at approximately 375 K? (6.03) 

17.	Using the diagram to the right, identify the process is occurring at each number. (6.03)

18.	Using the diagram in #17, identify the numbers that are associated with a decrease of kinetic energy. (6.03) 

19.	Explain why it is bad to overheat compressed cans of gas (i.e. spray paint cans). (6.04) 

20.	Which gas laws have inversely proportional relationships? (6.04)  

21.	What will most likely happen to the number of collisions of gas particles when the pressure decreases? Assume all other variables are held constant. (6.04)

22.	The pressure of a gas is 1.0 atm, the volume is 3.0 L, and the temperature is 200 K. A chemist changes one factor while keeping another constant so that the new pressure is 2.0 atm. Could the new set of conditions be that the final temperature is 375 K while keeping volume constant? Justify your answer. (6.04)

23.	The pressure of a gas is 1.5 atm, the temperature is 300 K and the volume is 2.3 L. A chemist keeps one of the variables the same while changing another.  If she were to decrease the temperature to 150 K while keeping the pressure constant, would the new volume increase or decrease and by what factor?  (6.04) 

24.	A sample of gas occupies a volume of 255 mL at a temperature of 375 K. At what temperature will this sample of gas occupy a volume of 300. mL? Show all of the work used to solve this problem. (6.04) Note:  Be able to solve a problem from all the gas laws from this lesson: Charles’s, Boyle’s, Avogadro’s and Gay-Lussac’s.

 Essay format questions:
25.	Using the kinetic molecular theory, describe what happens when gas from a 1-liter container is transferred to a 2-liter container.  (6.02).

26.	Student A sprayed perfume in a cold room and it took 30 seconds for it to disperse throughout the room. Student B sprayed perfume in a heated room and it took 10 seconds for it to disperse throughout the room.  Based on the KMT, compare these two rooms with respect to temperature, kinetic energy, particle motion and velocity.  (6.02)

Honors Extension (MC & Essay format):
27.	(6.06H) What is the volume of 1 mole of oxygen gas (O2) at standard temperature and pressure (STP)? 

28.	(6.06H) How many grams of oxygen gas (O2) need to be combusted to produce 9.50 L water vapor at 273 K and 1.30 atm? Show all of the work used to solve this problem.  CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (g)

29.	(6.06H) A chemist reacted 4.50 liters of CH4 gas with oxygen gas in the laboratory to form CO2 gas and water vapor. Use the ideal gas law equation to determine the mass of O2 that reacted with CH4 at 275 K and 0.75 atm. CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (g)

30.	(6.06H) What is the volume of 12.57 grams of He gas at STP?

31.	(6.06H) Assuming all volume measurements are made at the same temperature and pressure, how many liters of carbon dioxide gas can be produced when 12.8 liters of oxygen gas react with excess carbon monoxide? Show all of the work used to solve this problem.      2CO(g) + O2 (g) → 2CO2 (g)