Final NB 2016-2017 Turley

Question 1 Explanation:
In question 1 the answer is B A catalyst was added to trial #2 because if
we take a look at the trials in the graph we can see that trial A requires
way more energy than trail 2 to achieve its pathway to reaction. If we look
at the two different pathways we could assume that the factor that
changed the energy pathway in trial 2 was a catalyst. A catalyst is, “a
substance that enables a chemical reaction to proceed at a usually faster
rate or under different conditions (as at a lower temperature) than
otherwise possible” (Merriam Webster). In addition to this by looking at
answer A, which states, Heat was added to trial #2, we can see that this
would help the reaction, but not as much as what happened when the
catalyst was added. In addition, answer C and D are wrong because if
trial 2 was stirred or cooled it would not have the same effect of which
occurred in trial 2.
Question 2 Explanation:
For question 2 the answer is C adding a catalyst to the reaction because in any chemical reaction
adding a catalyst will help decrease the amount of energy need for the reaction. So if our goal is
trying to increase the rate at which the reaction will occur, it would be best to add a catalyst. In
addition to this the reason it’s not A, B, or D is because if we were to add pressure to the chemical
reaction it wouldn’t speed it up, either would decreasing the temperature because by doing so it
would only decrease the rate of the reaction. In addition to this by decreasing the concentration it
would only increase the solubility rather than increase the reaction process.
Question 3 Explanation:
For question 3 the answer is C, the average kinetic energy
increases, so the likelihood of more effective collisions between
ions increases, because this best defines how increasing the
temperature increases the rate of the reaction. If we were to
look at the other answers we would see that the rate of
temperature does not affect the amount of concentrations,
pressure, or the stability of systems at higher temperatures. C is
correct because is best and correctly explains how the increase of temperatures increase the rate of
the reaction.
Question 4:
For question 4 the answer is D, D increasing surface area
enables more reactant particles to collide, because if were
able to increase the size at which a reaction occurs it would
have allowed there to be more particles collide and more
space for the concentrate to dissolve or disperse within. If we
look at B and C we can tell those answers are insufficient to
the question asked because by changing the surface area, it
has no effect to the electro negativity of particles nor the
concentration of reaction particles. Lastly, it also has no effect
to the conductivity of reactant particles because by increasing the surface are you are only allowing
the ability for more particles to collide.
Question 5:
For question 5 the answer is D, decreasing the temperature, because in the chemical reaction shown
above a catalyst is shown already being added to the reaction. So by decreasing the temperature
with the already added catalyst we would be increasing the rate of the reaction further. We can also
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