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Chapter 17 Exam

Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 1. 
Examining a chemical system before and after a reaction reveals the
a.
net chemical change.
c.
intermediates.
b.
reaction mechanism.
d.
activated complex.
 

 2. 
In the reaction represented by the following equation, a possible intermediate is H2(g) + I2(g) mc002-1.jpg 2HI(g)
a.
H2.
c.
H2I.
b.
HI.
d.
I2.
 

 3. 
What is the overall equation for the formation of hydrogen iodide from its elements?
a.
mc003-1.jpg mc003-2.jpg mc003-3.jpg
b.
mc003-4.jpg mc003-5.jpg mc003-6.jpg
c.
mc003-7.jpg mc003-8.jpg mc003-9.jpg
d.
mc003-10.jpg mc003-11.jpg mc003-12.jpg
 

 4. 
What is the initial step in the formation of hydrogen iodide from its elements?
a.
mc004-1.jpg mc004-2.jpg mc004-3.jpg
b.
mc004-4.jpg mc004-5.jpg mc004-6.jpg
c.
mc004-7.jpg mc004-8.jpg mc004-9.jpg
d.
mc004-10.jpg mc004-11.jpg mc004-12.jpg
 

 5. 
A homogeneous reaction is one in which the
a.
reactants and products are in the same phase.
b.
reactants and products are in a different phase.
c.
activated complex and intermediates are in a different phase.
d.
one reactant is in a solid phase and another reactant is in a liquid phase.
 

 6. 
If colliding molecules have an orientation that favors reaction, they have
a.
the correct angles and distances between atoms.
b.
sufficient energy for each molecule.
c.
speeds that are neither too fast nor too slow.
d.
entropy values in the proper range.
 

 7. 
Which attempts to explain chemical reactions and physical interactions of molecules?
a.
chemical kinetics
c.
thermodynamics
b.
collision theory
d.
thermochemistry
 

 8. 
A short-lived structure formed during a collision is a(n)
a.
reagent.
c.
activated complex.
b.
catalyst.
d.
inhibitor.
 

 9. 
What is the name of the energy needed to lift reactants from the energy trough?
a.
free energy
c.
kinetic energy
b.
activation energy
d.
energy of reaction
 

 10. 
mc010-1.jpg is positive for
a.
an endothermic reaction.
c.
an inhibited reaction.
b.
an exothermic reaction.
d.
a stable reaction.
 

 11. 
The activation energy for a reaction is the energy difference between the
a.
product and the intermediate.
c.
reactant and the activated complex.
b.
product and the reactant.
d.
reactant and the intermediate.
 

 12. 
Chemical kinetics studies
a.
the factors that affect the rate of reaction.
b.
the mathematical expressions for the rate of reaction.
c.
the factors that affect the rate of reaction and the mathematical expressions for the rate of reaction.
d.
the effect of quantum kinetics on chemical reactions.
 

 13. 
The decrease in reactant concentration per unit time in a reaction is a measure of the
a.
reaction rate.
c.
overall reaction.
b.
heterogeneous reaction.
d.
reaction mechanism.
 

 14. 
If the surface area of reactants is larger,
a.
the reaction rate is generally higher.
c.
the reaction rate is not affected.
b.
the reaction rate is generally lower.
d.
the rate-determining step is eliminated.
 

 15. 
Changing the pressure of a gas is another way of changing its
a.
temperature.
c.
surface area.
b.
concentration.
d.
composition.
 

 16. 
Catalysts generally affect chemical reactions by
a.
increasing the temperature of the system.
b.
increasing the surface area of the reactants.
c.
providing an alternate pathway with a lower activation energy.
d.
providing an alternate pathway with a higher activation energy.
 

 17. 
A substance that slows down chemical processes is called a(n)
a.
inhibitor.
c.
catalyst.
b.
reactant.
d.
indicator.
 

 18. 
In a net equation, catalysts
a.
are shown with the reactants.
b.
are shown with the products.
c.
are shown with both reactants and products.
d.
are not shown.
 

 19. 
The letter k in a rate law stands for
a.
a proportionality constant.
c.
temperature.
b.
concentration.
d.
reaction rate.
 

 20. 
The letter R in a rate law stands for
a.
a proportionality constant.
c.
temperature.
b.
concentration.
d.
reaction rate.
 

 21. 
The value of k in a rate law
a.
is the same under all conditions.
c.
varies with time.
b.
varies with concentration.
d.
varies with temperature.
 

 22. 
The letter n in a rate law stands for
a.
a proportionality constant.
c.
temperature.
b.
concentration.
d.
reaction rate.
 

 23. 
According to the rate law, the rate of a reaction and the concentration of reactants are always
a.
equal.
c.
negative.
b.
proportional.
d.
unable to be determined.
 

 24. 
The rate of a reaction does not depend on the concentration of the reactant A when the order of reactant A is
a.
zero.
c.
two.
b.
one.
d.
three.
 

 25. 
A reaction is zero order in reactant A and second order in reactant B. What happens to the reaction rate when the concentrations of both reactants are doubled?
a.
The reaction rate remains the same.
b.
The reaction rate increases by a factor of two.
c.
The reaction rate increases by a factor of four.
d.
The reaction rate increases by a factor of eight.
 



 
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