FINISHED_Final_Notebook_Jones

The Learning Goal for this section is: Explain how various factors, such as concentration,
temperature, and the presence of a catalyst affect the rate of a chemical reaction.
You are going to answer these 15 questions first in the order they are given to you. This will be a quiz grade. You are then going to explain the
chemical concepts that are used in each question. You can do this in the order given or group them by concepts. You can use your book or information
found on the internet but all information must be written in your own word. The font needs to be Arial 12. This is due on Monday April 24 by midnight in
the drop box. This document should be a 6-page pdf.
1. B. 6. B. 11. A.
2. C. 7. B. 12. D.
3. C. 8. D. 13. B.
4. D. 9. A. 14. D.
5. A. 10. B. 15. D.
1. This graph represents the change in energy for two laboratory trials of the same reaction.
Which factor could explain the energy difference between the trials?
A. Heat was added to trial #2.
B. A catalyst was added to trial #2.
C. Trial #1 was stirred.
D. Trial #1 was cooled.
Explanation: Colliding particles must have a certain amount of energy in order to cause a reaction;
this minimum amount of energy is called ​activation energy​. When the particles collide with the amount
of energy required (and in the proper orientation), they form what is called an ​activated complex​.
Enzymes lower the required activation energy for this reaction to occur. You could also raise the
temperature to speed up the reaction. In this case, because the initial amount of energy remained the
same, there was no increase or decrease in temperature, thus an enzyme must have been added.
2. Consider this balanced chemical equation:
Which will increase the rate of the reaction?
A. increasing pressure on the reaction
B. decreasing concentration of the reactants
C. adding a catalyst to the reaction
D. decreasing the temperature of the reaction
2H​2​O​2​
​(aq)​
→ 2H​2​O​(l)​
+ O​ 2​
​(g)
Explanation: Adding a catalyst to the reaction would increase the rate of reaction because decreasing
the concentration would accomplish the opposite effect --reducing the chance of collision between
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