Complete Whole Notebook

The Learning Goal for this section is:
The student will learn how the rate of a chemical reaction can be controlled, what the role of energy is
and why some reactions occur naturally and others do not.
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.C
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: IN the first trial, the amount of energy required for the reaction to take place is more than
the amount in the second trial. A catalyst reduces the activation energy for the reaction to take place.
Collisions only result in a reaction if the particles collide with a certain minimum energy called the
activation energy for the reaction. To increase the rate of a reaction you need to increase the number
of successful collisions. One possible way of doing this is to provide an alternative way for the
reaction to happen which has a lower activation energy.
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
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2H2O2 (aq) → 2H2O(l) + O2 (g)