Download chapters 16-17 test re

NAME _____________________________________________
PERIOD _________
DATE ____________________________
CHAPTERS 16-17 TEST REVIEW
Remember to show your work as well as units. You can use one 3x5 card (front and back) on the test
as notes. The only thing I will give you will be a Periodic Table.
Questions #1-10 are True or False. Write True or False on the blank next to each question.
1. _______ A chemical reaction rate is defined as a specific amount of time per change in
concentration of a reactant or product.
2. _______ The Atomic Theory states that atoms, ions, or molecules must collide in order to react
provided that they have enough kinetic energy to form an activated complex and have the right
orientation.
3. _______ A low Ea means that relatively few collisions will have the required energy to produce
the activated complex, and the reaction rate is fast.
4. _______ Catalysts are enzymes that aren’t consumed in a chemical reaction, but they raise the
reaction rate by lowering the Ea.
5. _______ To calculate the overall reaction rate add the exponents of the reactants together.
6. _______ Intermediates are not consumed in a reaction mechanism.
7. _______ The rate-determining step is the fastest step in a reaction mechanism.
8. _______ At equilibrium the concentrations of both the reactants and the products become
constant, but not equal to each other.
9. _______ The equilibrium constant expression includes all states (solid, liquid, and gas).
10. _______ At equilibrium the rate of the forward reaction equals the rate of the reverse reaction.
Questions #11-30 are Multiple Choice. Write A, B, C, or D on the blank next to each question.
11. _____ Which of the following is not part of the Collision Theory?
a. Particles must spin
b. Particles must collide
c. Particles must have enough KE
d. Particles must have the right orientation
12. _____ What is another name for the transition state in a chemical reaction?
a. Activated complex
c. Intermediate
b. Elementary step
d. Activation energy
13. _____ Which of the following situations describes an exothermic reaction?
a. Energy of the reactants > Energy of the products
b. Activation energy is 0
c. Energy of the reactants < Energy of the products
d. Energy of the intermediates < Energy of the products
14. _____ Which of the following will not raise the reaction rate?
c. Raising the temperature
a. Increasing the concentration
b. Crushing a reactant into powder
d. Adding an inhibitor
15. _____ Which of the following lowers a reaction rate?
c. Intermediate
a. Catalyst
b. Activated complex
d. Inhibitor
16. _____ Which of the following is a key characteristic of a catalyst?
a. It is used up in the reaction
b. It doesn’t change the Ea
c. It becomes part of the final products
d. It isn’t used up in the reaction
17. _____ What is the primary goal when wanting to raise a reaction rate?
a. Raise the temperature
c. Increase the number of collisions
b. Increase the volume
d. Increase the surface area
18. _____ What is the overall reaction order for a reaction between A and B which has a rate law of
rate = k[A][B]2?
a. First
c. Third
b. Second
d. Fourth
19. _____ Reactant A is second order. What will happen to the reaction rate if the concentration of
A is doubled and all other concentrations stay the same?
a. It will double.
c. It will stay the same.
b. It will quadruple.
d. It will triple.
20. _____ Which of the following is the rate-determining step?
a. Fastest step
c. First step
b. Slowest step
d. Last step
21. _____ Which of the following is not included in an equilibrium constant expression?
a. Solids
c. Gases
b. Aqueous solutions
d. None of the above
22. _____ Which of the following is present at equilibrium?
a. Rate of forward rxn = Rate of reverse rxn
b. Rate of forward rxn > Rate of reverse rxn
c. Rate of forward rxn < Rate of reverse rxn
d. Equilibrium doesn’t depend on rate
23. _____ When are the products favored at equilibrium?
a. Keq < 1
c. Keq > 1
b. Keq = 1
d. Keq = 0
24. _____ Increasing the pressure or decreasing the volume will push the equilibrium towards the
side of the reaction that has what amount of moles of gas?
a. More
c. Fewer
b. The Same
d. Twice as much
25. _____ What is the equilibrium constant for the reaction between nitrogen gas and hydrogen
gas to form gaseous ammonia if [NH3] = 0.933 mol/L, [N2] = 0.533 mol/L, and [H2] = 1.600
mol/L?
a. 3.99
c. 0.229
b. 0.399
d. 39.99
26. _____ Which of the following is the equilibrium constant expression for FeO(s) + CO(g) ⇌ Fe(s)
+ CO2(g)?
a. Keq =
b. Keq =
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ሾ஼ைమ ሿ
ሾ஼ைమ ሿ
ሾ஼ைሿ
ሾி௘ሿሾ஼ை ሿ
మ
c. Keq = ሾி௘ைሿሾ஼ைሿ
d. Keq =
ሾி௘ைሿሾ஼ைሿ
ሾி௘ሿሾ஼ைమ ሿ
27. _____ Which of the following is the solubility product constant expression for copper (II)
hydroxide?
a. Ksp = [Cu2+][2OH-]
c. Ksp = [Cu2+][OH-]2
b. Ksp = 2[Cu][OH]
d. Ksp = [Cu+][OH-]2
28. _____ Which of the following is the common ion of both NaCl and HCl?
a. Na+
c. Cl2b. H+
d. Cl29. _____ Which of the following describes the lowering of the solubility of a substance because of
the presence of a common ion?
a. Common Ion Effect
c. Ion Reaction
b. Solubility Lowering
d. Collision Theory
30. _____ A 100.5 mL intravenous (IV) solution contains 5.10 g of glucose (C6H12O6). What is the
molarity of this solution?
a. 0.282 M
c. 2820 M
b. 282 M
d. 28.2 M
Questions #31-40 are Short Answer or Labeling. Answer each question as completely as possible.
31. In the figure below, identify each of the labels 1, 2, 3, 4, and 5 as one of the following: activated
complex, intermediate, reactants, or products.
32. A two-step mechanism has been proposed for the decomposition of nitryl chloride (NO2Cl).
What is the overall reaction? Identify any intermediates in the reaction sequence and explain
why they are intermediates.
a. Step 1: NO2Cl(g) → NO2(g) + Cl(g)
b. Step 2: NO2Cl(g) + Cl(g) → NO2(g) + Cl2(g)
33. In the gas-phase reaction, I2 + Cl2 → 2ICl, [I2] changes from 0.400M at 0.00 min to 0.300M at
4.00 min. Calculate the average reaction rate in moles of I2 consumed per liter per minute.
34. The rate law for the reaction 2NO(g) + O2(g) → 2NO2 is second order in O2 and third order
overall. What is the rate law for the reaction?
35. Assume that the rate law for a generic chemical reaction is rate = [A][B]3. What is the reaction
order in A, the reaction order in B, and the overall reaction order?
36. Calculate Keq for the following equilibrium: CO(g) +3H2(g) ⇌ CH4(g) + H2O(g) if [CO] = 0.0613
mol/L, [H2] = 0.1839 mol/L, [CH4] = 0.0387 mol/L, and [H2O] = 0.0387 mol/L.
37. The following reaction is first order in H2 and second order in NO with a rate constant of 2.90 x
102 (L2/(mol2●s)). 2NO(g) + H2(g) → N2O(g) + H2O(g). Calculate the instantaneous rate when the
reactant concentrations are [NO] = 0.002M and [H2] = 0.004M.
38. Le Chatelier’s Principle. Complete the following table by writing left, right, or none for the
equilibrium shift, and decreases, increases, or remains the same for the concentrations of each
reactant and product.
Heat + H2(g) + I2(g) ⇌ 2HI(g)
Stress
Add H2
Equilibrium Shift
Right
[H2]
X
Add I2
[I2]
Decreases
[HI]
Increases
X
Add HI
X
Remove H2
X
Remove I2
X
Remove HI
X
Increase Temperature
Decrease Temperature
Increase Pressure
Decrease Pressure
39. Stoichiometry Review. How many grams of CH4 are needed to produce 50.0 g of CHCl3
according to the following chemical reaction (hint: make sure you balance the equation first!)?
CH4 + Cl2 → CHCl3 + HCl
40. Naming Review. Complete the following table.
Compound Name
Compound Formula
Sulfuric Acid
B2O4
Copper (II) nitrate
CaCO3
Trinitrogen monosulfide
Is it ionic, molecular, or an acid?