Name:     ID: 
 
    Email: 

CHEM 1212 Practce Final Exam - Spring Term 2005  50 points

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

 1. 
Ideally, collligative properties depend only on
a.
the identity of the solute in a solution.
b.
the number of solute particles per solvent molecule in a solution.
c.
the temperature of a solution.
d.
the charge of the ions dissolved in solution.
e.
the gas pressure above the surface of a solution.
 

 2. 
What is the definition of molality?
a.
moles of solute per liter of solution
b.
grams of solute per kg of solution
c.
grams of solute per kg of solvent
d.
moles of solute per kg of solvent
e.
moles of solute per liter of solvent
 

 3. 
To prepare approximately 1 liter of a solution that is 4.75% by mass NaCl, one should
a.
dissolve 4.75 g NaCl in water up to a total volume of 1.00 L.
b.
dissolve 47.5 g NaCl in 1.00 ´ 103 g water.
c.
dissolve 47.5 g NaCl in 952.5 g water.
d.
dissolve 952.5 g NaCl in 47.5 g water.
e.
dissolve 46.5 g NaCl in 1.00 kg water.
 

 4. 
The molality of a sodium nitrate solution is 1.44 m. What is the mole fraction of NaNO3? The molar mass of NaNO3 is 85.06 g/mol; the molar mass of water is 18.02 g/mol.
a.
0.0253
b.
0.0571
c.
0.122
d.
0.688
e.
2.21
 

 5. 
Concentrated hydrofluoric acid is 49.0% HF by mass and has a density of 1.30 g/mL. What is the molarity of concentrated HF?
a.
12.1 M
b.
17.4 M
c.
18.8 M
d.
24.5 M
e.
31.8 M
 

 6. 
Equal masses of water and ethylene glycol are mixed. What is the concentration of ethylene glycol in units of molality? The molar mass of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively.
a.
3.21 m
b.
6.92 m
c.
11.1 m
d.
16.1 m
e.
18.2 m
 

 7. 
Which of the following liquids are likely to be miscible with water: 1-propanol, carbon tetrachloride, cyclohexane, and formic acid (HCO2H)?
a.
1- propanol and cyclohexane
b.
carbon tetrachloride and cyclohexane
c.
cyclohexane and formic acid
d.
carbon tetrachloride and formic acid
e.
1-propanol and formic acid
 

 8. 
Which of the following actions will increase the equilibrium concentration of a gas in water?

1. increasing the temperature of the water
2. increasing the volume water
3. increasing the pressure of the gas above the liquid
a.
1 only
b.
2 only
c.
3 only
d.
1 and 3
e.
1, 2, and 3
 

 9. 
The vapor pressure of pure water at 35ºC is 42.2 mm Hg. What is the vapor pressure of a mixture of 15 g sucrose (C12H22O11, molar mass 342.3 g/mol) and 85 g water?
a.
7.45 mm Hg
b.
21.8 mm Hg
c.
35.9 mm Hg
d.
40.6 mm Hg
e.
41.8 mm Hg
 

 10. 
Which of the following aqueous solutions should have the lowest boiling point?
a.
0.4 m MgBr2
b.
0.5 m Na2SO4
c.
0.75 m NaCl
d.
1 m KI
e.
2 m LiBr
 

 11. 
If 1.928 g KNO3 is dissolved in enough water to make 250.0 mL of solution, what is the molarity of potassium nitrate?
a.
6.912 ´ 10-4 M
b.
4.767 ´ 10-3 M
c.
7.627 ´ 10-2 M
d.
1.297 ´ 10-1 M
e.
7.712 M
 

 12. 
Which of the following directions correctly describe the preparation of 0.500 L of 0.150 M NaOH from a 6.00 M stock solution?
a.
Dilute 0.200 L of 6.00 M NaOH to a volume of 0.500 L.
b.
Dilute 12.5 mL of 6.00 M NaOH to a volume of 0.500 L.
c.
Combine 0.200 L of 6.00 M NaOH with 0.500 L of water.
d.
Dilute 475 mL of 6.00 M NaOH to a volume of 0.500 L.
e.
Combine 12.5 mL of 6.00 M NaOH with 0.500 L of water.
 

 13. 
Which of the following properties of water can be attributed to hydrogen bonding?

1. high melting point
2. high heat of vaporization
3. low vapor pressure
4. high surface tension
a.
1 and 3
b.
2 and 3
c.
2, 3, and 4
d.
1, 3, and 4
e.
1, 2, 3, and 4
 

 14. 
Which of the following processes is exothermic?
a.
solid to gas
b.
liquid to gas
c.
liquid to solid
d.
solid to liquid
e.
none of the above
 

 15. 
Which process requires the greatest exothermic change in enthalpy for water?
a.
vaporization
b.
condensation
c.
sublimation
d.
melting
e.
fusion
 

 16. 
The normal boiling point is defined as
a.
the pressure of a gas when its temperature reaches 373.15 K.
b.
the temperature at which the vapor pressure of a substance equals 1 atm.
c.
the temperature at which water boils.
d.
the pressure at which a liquid boils at 273.15 K.
e.
the sum of the enthalpies of vaporization and fusion at 298 K.
 

 17. 
Which of the following statements are correct?

1. A liquid boils when its vapor pressure is equal to the pressure above its surface.
2. Above the critical pressure, only the solid phase of a pure substance can exist.
3. The gas, liquid, and solid phases can all coexist at the critical point.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
1 and 3
 

 18. 
Which of the following gases can be liquefied at 25ºC?

Gas
boiling pt.
critical temp.
N2
-196ºC
-147ºC
Cl2
-34ºC
144ºC
O2
-183ºC
-119ºC
a.
N2 only
b.
Cl2 only
c.
O2 only
d.
Cl2 and O2
e.
N2 and O2
 

 19. 
In the unit cell below, element X is within the cell and element Y is at the corners. What is the formula for this compound?

1212finals05_files/i0200000.jpg
a.
XY
b.
XY2
c.
XY4
d.
XY8
e.
X2Y
 

 20. 
Which of the following statements concerning the phase diagram below are correct?

1212finals05_files/i0210000.jpg

1. Moving from point A to B results in a phase transition from solid to liquid.
2. Point D lies at the critical point.
3. At point C, liquid and gas phases coexist at equilibrium.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 3
e.
2 and 3
 

 21. 
Which of the statements concerning relative rates of reaction is correct for the decomposition of dinitrogen pentaoxide?

2 N2O5(g) ® 4 NO2(g) + O2(g)
a.
The rate of disappearance of N2O5 is 1/2 the rate of appearance of O2.
b.
The rate of appearance of NO2 is 1/4 the rate of appearance of O2.
c.
The rate of disappearance of N2O5 is 1/2 the rate of appearance of NO2.
d.
The rate of appearance of NO2 equals the rate of appearance of O2.
e.
The rate of disappearance of N2O5 equals the rate of appearance of NO2.
 

 22. 
Given the initial rate data for the reaction A + B ® C, determine the rate expression for the reaction.

[A], M
[B], M
D[C]/Dt (initial) M/s
0.25
0.15
1.23 ´ 10-3
0.25
0.25
3.42 ´ 10-3
0.50
0.15
2.46 ´ 10-3
a.
1212finals05_files/i0230000.jpg = 0.0328[A][B]
b.
1212finals05_files/i0230001.jpg = 0.0547[A][B]
c.
1212finals05_files/i0230002.jpg = 0.219[A][B]2
d.
1212finals05_files/i0230003.jpg = 0.0547[A][B]2
e.
1212finals05_files/i0230004.jpg = 0.219[A]2[B]
 

 23. 
Given the initial rate data for the reaction A + B ® C, determine the rate expression for the reaction.

[A], M
[B], M
D[C]/Dt (initial) M/s
0.125
0.105
1.23 ´ 10-1
0.125
0.315
3.69 ´ 10-1
0.250
0.105
1.23 ´ 10-1
a.
1212finals05_files/i0240000.jpg = 75.0[A]2[B]
b.
1212finals05_files/i0240001.jpg = 1.17[B]
c.
1212finals05_files/i0240002.jpg = 1.17[A]2[B]
d.
1212finals05_files/i0240003.jpg = 11.2[B]2
e.
1212finals05_files/i0240004.jpg = 11.2[A]
 

 24. 
What is the overall order of the reaction

CO(g) + NO2(g) ® CO2(g) + NO(g)

if it proceeds via the following rate expression?

1212finals05_files/i0250000.jpg = k[CO][NO2]
a.
zero-order
b.
first-order
c.
second-order
d.
third-order
e.
fourth-order
 

 25. 
For the reaction A ® B, the rate law is

1212finals05_files/i0260000.jpg = k[A]

What are the units of the rate constant where time is measured in seconds?
a.
1212finals05_files/i0260001.jpg
b.
M • s
c.
1212finals05_files/i0260002.jpg
d.
1212finals05_files/i0260003.jpg
e.
1212finals05_files/i0260004.jpg
 

 26. 
Which of the following factors often affect the value of the rate constant of a chemical reaction?

1. changes in the concentrations of reactants
2. changes in the temperature of the system
3. the addition of a catalyst
a.
1 only
b.
2 only
c.
3 only
d.
2 and 3
e.
1, 2, and 3
 

 27. 
The reaction of NO(g) and O2(g) produces NO2(g).

2 NO(g) + O2(g) ® 2 NO2(g)

The reaction is second-order with respect to NO(g) and first-order with respect to O2(g). At a given temperature, the rate constant, k, equals 5.7 ´ 103 M-2s-1. What is the rate of reaction when the initial concentrations of NO and O2 are both 0.020 M?
a.
1.4 ´ 10-9 M/s
b.
4.6 ´ 10-2 M/s
c.
9.1 ´ 10-2 M/s
d.
2.3 ´ 100 M/s
e.
7.1 ´ 108 M/s
 

 28. 
What determines the exponents in a rate law?

1. experimentation
2. the coefficients in the balanced equation
3. the concentrations of the reactants
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
2 and 3
 

 29. 
The half-life of a first-order decomposition reaction is 188 seconds. If the initial concentration of reactant is 0.524 M, what is the concentration of reactant after 752 seconds?
a.
0.0164 M
b.
0.0328 M
c.
0.0665 M
d.
0.133 M
e.
0.266 M
 

 30. 
Which of the following changes generally lead to greater reaction rates?

1. Increasing the temperature
2. Decreasing the concentration of a reactant
3. Adding a catalyst
a.
1 only
b.
2 only
c.
1 and 3
d.
2 and 3
e.
1,2, and 3
 

 31. 
In general, as the temperature increases, the rate of a chemical reaction
a.
decreases due to fewer collisions with proper molecular orientation.
b.
decreases for endothermic reactions.
c.
decreases for exothermic reactions.
d.
increases due a greater number of effective collisions.
e.
increases due to a lowering of activation energy.
 

 32. 
The effect of a catalyst is to
a.
lower the activation energy of a reaction.
b.
increase the energy of the products.
c.
increase the energy of the reactants.
d.
increase the number of collisions between reactants.
e.
decrease the change in enthalpy of a reaction.
 

 33. 
The elementary steps for the catalyzed decomposition of dinitrogen monoxide are shown below. Identify the catalyst in the reaction.

N2O(g) + NO(g) ® N2(g) + NO2(g)
2 NO2(g) ® 2 NO(g) + O2(g)
a.
N2
b.
NO
c.
N2O
d.
NO2
e.
O2
 

 34. 
In basic solution, (CH3)3CCl reacts according to the equation below.

(CH3)3CCl + OH- ® (CH3)3COH + Cl-

The accepted mechanism for the reaction is

(CH3)3CCl ® (CH3)3C+ + Cl-
(slow)
(CH3)3C+ + OH- ® (CH3)3COH
(fast)

What is the rate law for the reaction?
a.
rate = k[(CH3)3CCl]
b.
rate = k[(CH3)3CCl]2
c.
rate = k[(CH3)3C+][OH-]
d.
rate = k[(CH3)3CCl][OH]
e.
rate = k[(CH3)3CCl][Cl-][OH-]
 

 35. 
Nitrogen monoxide reacts with chlorine to produce NOCl.

2 NO(g) + Cl2(g) ® 2 NOCl(g)

A proposed mechanism for this reaction is

NO(g) + NO(g) 1212finals05_files/i0360000.jpg N2O2(g)
(fast, equilibrium)
N2O2(g) + Cl2(g) ® 2 NOCl(g)
(slow)

What is a rate law that is consistent with this mechanism?
a.
rate = k[NO][Cl2]
b.
rate = k[[NO]2
c.
rate = k[N2O2][Cl2]
d.
rate = k[NO][Cl2]2
e.
rate = k[NO]2[Cl2]
 

 36. 
Which of the following statements concerning equilibrium constants are true?

1. Kinetically fast reactions always have large equilibrium constants.
2. Temperature has no effect on an equilibrium constant.
3. Reactant favored reactions have negative equilibrium constants.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
none of above
 

 37. 
A large equilibrium constant
a.
is obtained with catalysts.
b.
indicates the formation of products is favored.
c.
is common for equilibria at high temperatures.
d.
indicates that a reaction has a small activation barrier.
e.
indicates that a reaction has a large rate constant.
 

 38. 
Write the expression for Kc for the reaction below.

Mg3(PO4)2(s) 1212finals05_files/i0390000.jpg 3 Mg2+(aq) + 2 PO43-(aq)
a.
1212finals05_files/i0390001.jpg
b.
1212finals05_files/i0390002.jpg
c.
1212finals05_files/i0390003.jpg
d.
1212finals05_files/i0390004.jpg
e.
1212finals05_files/i0390005.jpg
 

 39. 
Write the expression for K for the acid reaction below.

HF(aq) + H2O(ª) 1212finals05_files/i0400000.jpg F-(aq) + H3O+(aq)
a.
1212finals05_files/i0400001.jpg
b.
1212finals05_files/i0400002.jpg
c.
1212finals05_files/i0400003.jpg
d.
1212finals05_files/i0400004.jpg
e.
1212finals05_files/i0400005.jpg
 

 40. 
A gaseous mixture of NO2 and N2O4 is in equilibrium. If the concentration of N2O4 is 3.5 ´ 10-3 M, what is the concentration of NO2?

2 NO2(g) 1212finals05_files/i0410000.jpg N2O4(g)      Kc = 170
a.
2.1 ´ 10-5 M
b.
4.5 ´ 10-3 M
c.
7.1 ´ 10-2 M
d.
2.2 ´ 102 M
e.
4.9 ´ 104 M
 

 41. 
We place 0.064 mol N2O4(g) in a 4.00 L flask at 200. After reaching equilibrium, the concentration of NO2(g) is 0.0030 M. What is Kc for the reaction below?

N2O4(g) 1212finals05_files/i0420000.jpg 2 NO2(g)
a.
3.6 ´ 10-5
b.
4.7 ´ 10-5
c.
5.6 ´ 10-4
d.
6.2 ´ 10-4
e.
1.9 ´ 10-1
 

 42. 
We place 3.2 mol PCl5 in a 2.0 L flask and allow it to reach equilibrium at a given temperature. What is the final concentration of Cl2 in the flask?

PCl5(g) 1212finals05_files/i0430000.jpg PCl3(aq) + Cl2(g)          Kc = 0.47
a.
0.11 M
b.
0.27 M
c.
0.32 M
d.
0.55 M
e.
0.66 M
 

 43. 
Consider the reaction A(g)1212finals05_files/i0440000.jpg2 B(g) where Kp = 4.0. If 2.0 mol A and 3.0 mol B are introduced into a 1.0 L flask, what change in concentrations (if any) will occur in time?
a.
[A] increases and [B] increases
b.
[A] increases and [B] decreases
c.
[A] decreases and [B] increases
d.
[A] decreases and [B] decreases
e.
[A] and [B] remain unchanged
 

 44. 
Assume that the following endothermic chemical reaction is at equilibrium.

C(s) + H2O(g) 1212finals05_files/i0450000.jpg H2(g) + CO(g)

All of the following will increase the ratio of products to reactants in the equilibrium mixture EXCEPT
a.
increasing the temperature.
b.
increasing the volume.
c.
decreasing the pressure
d.
addition of solid carbon.
e.
removal of a gaseous product.
 

 45. 
The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process.

N2(g) + 3 H2(g) 1212finals05_files/i0460000.jpg 2 NH3(g)
H = -92.2 kJ

Which of the following would drive the equilibrium system to the left?
a.
addition of hydrogen
b.
removal of ammonia
c.
increasing the pressure
d.
decreasing the temperature
e.
removal of nitrogen
 

 46. 
In which of the following equilibrium systems would a decrease in volume have no effect on the concentrations of products and reactants?
a.
CaCO3(s)1212finals05_files/i0470000.jpgCaO(s) + CO2(g)
b.
N2(g) + 3 H2(g)1212finals05_files/i0470001.jpg2 NH3(g)
c.
H2(g) + CO2(g)1212finals05_files/i0470002.jpgCO(g) + H2O(g)
d.
3 O2(g)1212finals05_files/i0470003.jpg2 O3(g)
e.
2 H2O2(g)1212finals05_files/i0470004.jpg2 H2O(g) + O2(g)
 

 47. 
According to the Brønsted-Lowry definition, a base
a.
increases the H3O+ concentration in a solution.
b.
increases the OH- concentration in a solution.
c.
is a proton donor.
d.
is a proton acceptor.
e.
has a lone pair of electrons that can bond to a proton.
 

 48. 
All of the following are weak acids EXCEPT
a.
HF
b.
CH3CO2H
c.
HBr
d.
NH4+
e.
HCN
 

 49. 
In the following reaction

HCO3-(aq) + NH3(aq) 1212finals05_files/i0500000.jpg CO32-(aq) + NH4+(aq)
a.
HCO3- is an acid and NH3(aq) is its conjugate base.
b.
HCO3- is an acid and CO32- is its conjugate base.
c.
NH3 is an acid and HCO32- is its conjugate base.
d.
NH3 is an acid and NH4+ is its conjugate base.
e.
NH4+ is an acid and CO32- is its conjugate base.
 

 50. 
The conjugate acid of OH- is
a.
H3O+
b.
H2O
c.
OH-
d.
O2-
e.
H-
 

 51. 
What is the conjugate acid of HPO42-(aq)?
a.
H3PO4
b.
H2PO4-
c.
PO42-
d.
H3O+
e.
OH-
 

 52. 
What is the OH- concentration of a solution with a pH of 3.75?
a.
5.2 ´ 10-13 M
b.
5.6 ´ 10-11 M
c.
4.9 ´ 10-7 M
d.
1.8 ´ 10-4 M
e.
3.8 ´ 10-2 M
 

 53. 
Which of the following chemical reactions corresponds to the base ionization constant, Kb, for ammonia?
a.
NH3(aq) + H2O(ª) 1212finals05_files/i0540000.jpg NH4+(aq) + OH-(aq)
b.
NH4+(aq) + H2O(ª) 1212finals05_files/i0540001.jpg NH3(aq) + H3O+(aq)
c.
NH4+(aq) + OH-(aq) 1212finals05_files/i0540002.jpg NH3(aq) + H2O(ª)
d.
NH3(aq) + OH-(aq) 1212finals05_files/i0540003.jpg NH2-(aq) + H2O(ª)
e.
NH3(aq) + H3O+(aq) 1212finals05_files/i0540004.jpg NH4+(aq) + H2O(ª)
 

 54. 
Which of the following weak acids has the strongest conjugate base?
a.
acetic acid, Ka = 1.8 ´ 10-5
b.
benzoic acid, Ka = 6.3 ´ 10-5
c.
dihydrogen phosphate ion, Ka = 6.2 ´ 10-8
d.
formic acid, Ka = 1.8 ´ 10-4
e.
hydrocyanic acid, Ka = 4.0 ´ 10-10
 

 55. 
What is the pH of a 0.050 M solution of formic acid? (Ka for HCO2H = 1.8 ´ 10-4)
a.
2.54
b.
2.91
c.
3.21
d.
4.07
e.
5.99
 

 56. 
What is the pH of a 0.75 M solution of sodium cyanide, NaCN? (Kb for CN- =
2.5 ´ 10-5)
a.
2.36
b.
4.33
c.
9.58
d.
10.04
e.
11.64
 

 57. 
Which of the following chemical reactions corresponds to Ka2 for phosphoric acid?
a.
HPO42-(aq) + H2O(ª) 1212finals05_files/i0580000.jpg PO43-(aq) + H3O+(aq)
b.
PO43-(aq) + H2O(ª) 1212finals05_files/i0580001.jpg HPO42-(aq) + OH-(aq)
c.
H3PO4(aq) + H2O(ª) 1212finals05_files/i0580002.jpg H2PO4-(aq) + H3O+(aq)
d.
H3PO4(aq) + 2 H2O(ª) 1212finals05_files/i0580003.jpg HPO42-(aq) + 2 H3O+(aq)
e.
H2PO4-(aq) + H2O(ª) 1212finals05_files/i0580004.jpg HPO42-(aq) + H3O+(aq)
 

 58. 
What is the pH of 0.50 M H3PO4? (Ka1 = 7.5 ´ 10-3, Ka2 = 6.2 ´ 10-8, Ka3 = 3.6 ´ 10-13)
a.
0.97
b.
1.24
c.
2.67
d.
5.15
e.
6.33
 

 59. 
Of the following salts, which one forms a 0.1 M solution with the highest pH?
a.
KCl
b.
NH4Cl
c.
FeCl3
d.
KNO2
e.
Ca(NO3)2
 

 60. 
All of the following compounds are acids containing chlorine. Which compound is the weakest acid?
a.
HCl
b.
HClO
c.
HClO2
d.
HClO3
e.
HClO4
 

 61. 
We have a solution of ammonia. What is the effect of adding ammonium chloride to this solution?

1. The pH increases.
2. The concentration of NH3 increases.
3. The concentration of H3O+ increases
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
2 and 3
 

 62. 
What is the pH of a solution of 0.25 M acetic acid and 0.25 M sodium acetate? (Ka for CH3CO2H = 1.8 ´ 10-5)
a.
0.60
b.
2.12
c.
2.67
d.
4.74
e.
5.32
 

 63. 
Which of the following combinations would be the best to buffer the pH to 9.0?
a.
H3PO4 and H2PO4-, Ka = 7.5 ´ 10-3
b.
HNO2 and NO2-, Ka = 4.5 ´ 10-4
c.
CH3CO2H and CH3COO-, Ka = 18 ´ 10-5
d.
H2PO4- and HPO42-, Ka = 6.2 ´ 10-8
e.
NH4+ and NH3, Ka = 5.7 ´ 10-10
 

 64. 
All of the following will produce a buffer solution EXCEPT
a.
NH4Cl and NH3.
b.
HCN and KCN.
c.
NaHCO3 and Na2CO3.
d.
NaH2PO4 and Na2HPO4.
e.
NaOH and NaCl.
 

 65. 
Which of the following mathematical expressions is the Henderson-Hasselbalch equation?
a.
pH = pKa + log1212finals05_files/i0660000.jpg
b.
pKa = pH + lo1212finals05_files/i0660001.jpg
c.
pH = pKa + log1212finals05_files/i0660002.jpg
d.
pKa = pH - log1212finals05_files/i0660003.jpg
e.
None of the above equations is correct.
 

 66. 
All of the following statements concerning buffers are true EXCEPT
a.
buffers are resistant to changes in pH upon the addition of strong acids.
b.
buffers are resistant to changes in pH when diluted with water.
c.
the pH of a buffer is close to the pKa of the weak acid from which it is made.
d.
buffers contain appreciable quantities of a weak acid and its conjugate base.
e.
buffers are used as colored indicators in acid-base titrations.
 

 67. 
What is the pH of a buffer that results when 0.50 mole of H3PO4 is mixed with 0.75 mole of NaOH and diluted with water to 1.00 L? (Ka1 = 7.5 ´ 10-3, Ka2 = 6.2 ´ 10-8, Ka3 = 3.6 ´ 10-13)
a.
7.21
b.
7.45
c.
8.01
d.
8.23
e.
9.91
 

 68. 
If the ratio of base to acid in a buffer changes by a factor of 10, the pH of the buffer
a.
increases by 2.
b.
increases by 1.
c.
decreases by 1.
d.
decreases by 2.
e.
remains unchanged.
 

 69. 
Which one of the following conditions is true for a titration of a weak acid with a strong base?
a.
The equivalence point occurs at a pH greater than 7.
b.
The equivalence point occurs at a pH equal to 7.
c.
Equal volumes of acid and base are required to reach the equivalence point.
d.
A colored indicator with a pKa less than 7 should be used.
e.
The colored indicator should change color rapidly in the buffer region.
 

 70. 
Potassium hydrogen phthalate (molar mass = 204.2 g/mol) is used to standardize sodium hydroxide. If 22.10 mL of NaOH is required to titrate 0.6103 g KHP to the equivalence point, what is the concentration of the NaOH?

HC8H4O4-(aq) + OH-(aq) 1212finals05_files/i0710000.jpg C8H4O42-(aq) + H2O(ª)
a.
0.06605 M
b.
0.1352 M
c.
0.1514 M
d.
0.1617 M
e.
0.2762 M
 

 71. 
A 25.0 mL sample of vinegar is titrated with 0.0950 M NaOH. If the titration requires 35.8 mL of NaOH, what is the concentration of acetic acid in the vinegar?
a.
0.0663 M
b.
0.0971 M
c.
0.136 M
d.
0.329 M
e.
0.727 M
 

 72. 
Which of the following equations is the solubility product for Ca(IO3)2?
a.
Ksp = [Ca2+][I-]2[O2-]6
b.
Ksp = [Ca2+][I-]2[3O2-]2
c.
Ksp = [Ca2+][IO1212finals05_files/i0730000.jpg]
d.
Ksp = [Ca2+][IO1212finals05_files/i0730001.jpg]2
e.
Ksp = [Ca2+]2[IO1212finals05_files/i0730002.jpg]
 

 73. 
The solubility of BaSO4 is 1.05 ´ 10-5 mol/L. What is the value of Ksp for BaSO4?
a.
3.24 ´ 10-3
b.
6.48 ´ 10-3
c.
2.10 ´ 10-5
d.
1.10 ´ 10-10
e.
2.20 ´ 10-10
 

 74. 
The Ksp for BaF2 is 1.7 ´ 10-6. What is the concentration of Ba2+ in a saturated solution of BaF2?
a.
5.7 ´ 10-7 M
b.
1.7 ´ 10-6 M
c.
1.0 ´ 10-2 M
d.
1.3 ´ 10-3 M
e.
7.5 ´ 10-3 M
 

 75. 
The following anions can be separated by precipitation as silver salts: Cl-, Br-, I-, CrO42-. If Ag+ is added to a solution containing the four anions, each at a concentration of 0.10 M, in what order would they precipitate?

Compound
Ksp
AgCl
1.8 ´ 10-10
Ag2CrO4
9.0 ´ 10-12
AgBr
3.3 ´ 10-13
AgI
1.5 ´ 10-16
a.
AgCl®Ag2CrO4®AgBr®AgI
b.
AgI®AgBr®Ag2CrO4®AgCl
c.
Ag2CrO4®AgCl AgBr®AgI
d.
Ag2CrO4®AgI AgBr®AgCl
e.
AgI®AgBr®AgCl®Ag2CrO4
 

 76. 
If the reaction A + B 1212finals05_files/i0770000.jpg C has an equilibrium constant greater than one, which of the following statements is correct?
a.
The reaction is not spontaneous.
b.
The forward rate of reaction is fast.
c.
The backward rate of reaction is slow.
d.
The reaction is product favored.
e.
All of the above statements are correct.
 

 77. 
If a chemical reaction has a positive change in entropy, S, then
a.
the disorder of the system increases.
b.
the reaction is exothermic.
c.
heat goes from the system into the surroundings.
d.
the Gibbs free energy is negative.
e.
the reaction is spontaneous.
 

 78. 
Thermodynamics can be used to determine all of the following EXCEPT
a.
the direction in which a reaction is spontaneous.
b.
the extent to which a reaction occurs.
c.
the rate of reaction.
d.
the temperature at which a reaction is spontaneous.
e.
the enthalpy change of a reaction.
 

 79. 
A statement of the second law of thermodynamics is that
a.
spontaneous reactions are always exothermic.
b.
energy is conserved in a chemical reaction.
c.
the entropy of the universe is continually increasing.
d.
the enthalpy of reaction is the difference between product and reactant enthalpies.
e.
the Gibbs free energy is a function of both enthalpy and entropy.
 

 80. 
Of the following product-favored processes, which are endothermic?

1. the combustion of methane to produce water and carbon dioxide
2. the expansion of an ideal gas
3. the melting of ice at temperatures greater than 0ºC.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
2 and 3
 

 81. 
All of the following processes lead to an increase in entropy EXCEPT
a.
increasing the temperature of a gas.
b.
freezing a liquid.
c.
evaporating a liquid.
d.
forming mixtures from pure substances.
e.
chemical reactions that increase the number of moles of gas.
 

 82. 
Predict the signs of DH and DS for the evaporation of water at 35ºC.
a.
DH > 0 and DS > 0
b.
DH > 0 and DS < 0
c.
DH < 0 and DS > 0
d.
DH < 0 and DS < 0
e.
Not enough information is provided to answer this question.
 

 83. 
Predict the signs of DH, DS, and DG for the combustion of hydrogen gas at 25ºC.

2 H2(g) + O2(g) ® 2 H2O(ª)
a.
DH < 0, DS < 0, DG < 0
b.
DH < 0, DS > 0, DG < 0
c.
DH < 0, DS > 0, DG < 0
d.
DH > 0, DS < 0, DG < 0
e.
DH > 0, DS < 0, DG > 0
 

 84. 
Predict the signs of DH, DS, and DG for the melting of ice at 50ºC.
a.
DH < 0, DS < 0, DG < 0
b.
DH < 0, DS > 0, DG < 0
c.
DH < 0, DS > 0, DG < 0
d.
DH > 0, DS < 0, DG < 0
e.
DH > 0, DS > 0, DG < 0
 

 85. 
If DG < 0 for a reaction at all temperatures, then DS is ________ and DH is ________.
a.
positive, positive
b.
positive, negative
c.
zero, positive
d.
negative, positive
e.
negative, zero
 

 86. 
The dissolution of ammonium nitrate occurs spontaneously in water. As NH4NO3 dissolves, the temperature of the water decreases. What are the signs of H, S, and G for this process?
a.
DH < 0, DS < 0, DG < 0
b.
DH < 0, DS > 0, DG < 0
c.
DH < 0, DS > 0, DG < 0
d.
DH > 0, DS > 0, DG < 0
e.
DH > 0, DS < 0, DG > 0
 

 87. 
All of the following relationships are true EXCEPT
a.
DG1212finals05_files/i0880000.jpg = DH1212finals05_files/i0880001.jpg - TDS1212finals05_files/i0880002.jpg
b.
DG1212finals05_files/i0880003.jpg = - RT 1n(K)
c.
DS1212finals05_files/i0880004.jpg = DS1212finals05_files/i0880005.jpg + DS1212finals05_files/i0880006.jpg
d.
DH = DH1212finals05_files/i0880007.jpg + RT 1n(K)
e.
DG1212finals05_files/i0880008.jpg - TDS1212finals05_files/i0880009.jpg
 

 88. 
At what temperature would you expect a reaction to become spontaneous if DH = +67.0 kJ and DS = -131 J/K?
a.
T < -511 K
b.
T > 238 K
c.
T > 511 K
d.
The reaction will be spontaneous at any temperature.
e.
The reaction will NOT be spontaneous at any temperature.
 

 89. 
Calculate 1212finals05_files/i0900000.jpg for the reaction below at 25.0ºC

2 H2O2(ª) ® 2 H2O(ª) + O2(g)

given DG1212finals05_files/i0900001.jpg[H2O2(ª)] = -120.35 kJ/mol, DG1212finals05_files/i0900002.jpg [H2O(ª)] = -237.13 kJ/mol, DG1212finals05_files/i0900003.jpg[O2(g)] = 0 kJ/mol.
a.
714.96 kJ
b.
543.91 kJ
c.
-438.23 kJ
d.
-233.56 kJ
e.
-67.03 kJ
 

 90. 
If DGº< 0, then
a.
K >1
b.
K = 0
c.
K < 1
d.
K = 1
e.
K < 0
 

 91. 
For a chemical system, DGº and DG are equal when
a.
the equilibrium constant, K, equals 1.
b.
the equilibrium constant, K, equals 0.
c.
a system is at equilibrium.
d.
the reactants and products are in standard state concentrations.
e.
the reactant and products are in the gas phase.
 

 92. 
The equilibrium constant for a reaction at 298 K is 9.3 ´ 10-12. What is DGº? (R = 8.314 J/Kmol)
a.
2.54 kJ
b.
+2.54 kJ
c.
+5.28 kJ
d.
+62.9 kJ
e.
+87.1 kJ
 

 93. 
Given that

C(s) + O2(g) ® CO2(g)
DGº = -394.4 kJ
CO(g) + O2(g) ® CO2(g)
DGº = -257.2 kJ

calculate DGº for the following reaction.

C(s) + O2(g)® CO(g)
a.
651.6 kJ
b.
137.2 kJ
c.
+1.53 kJ
d.
+45.3 kJ
e.
+651.6 kJ
 

 94. 
Calculate for CaCO3 given the following information.

C(s) + O2(g) ® CO2(g)
DGº = -394.4 kJ
CaO(g) + CO2(g) ® CaCO 3(s)
DGº = -130.4 kJ
Ca(s) + O2(g) ® CaO(s)
DGº = -604.0 kJ
a.
1128.8 kJ
b.
340.0 kJ
c.
130.4 kJ
d.
+868.0 kJ
e.
+1128.8 kJ
 

 95. 
The following reaction occurs spontaneously.

2 H+(aq) + Ca(s) ® Ca2+(aq) + H2(g)

Write the balanced oxidation half-reaction.
a.
2 H+(aq) + 2 e- ® H2(g)
b.
2 H+(aq) ® H2(g) + 2 e-
c.
2 H+(aq) + Ca(s) ® 2 e-
d.
Ca(s) + 2 e- ® Ca2+(aq)
e.
Ca(s) ® Ca2+(aq) + 2 e-
 

 96. 
The following reaction occurs spontaneously,

3 Cu2+(aq) + 2 Fe(s) ® 2 Fe3+(aq) + 3 Cu(s)

Write the balanced reduction half-reaction.
a.
2 Fe(s) ® 2 Fe3+(aq) + 6 e-
b.
2 Fe(s) + 6 e- ® 2 Fe3+(aq)
c.
3 Cu2+(aq) + 6 e- ® 3 Cu(s)
d.
3 Cu2+(aq) ® 3 Cu(s) + 6 e-
e.
3 Cu2+(aq) + 2 Fe(s) + 6 e- ® 3Cu(s) + 2 Fe3+(aq)
 

 97. 
Write a balanced half-reaction for the oxidation of water.
a.
2 H2O(ª) ® O2(g) + 4 H+(aq) + 4 e-
b.
2 H2O(ª) ® H2(g) + 2 OH-(aq) + 2 e-
c.
H2O(ª) + 2 e- ® H2(g) + 2 OH-(aq)
d.
2 H2O(ª) + 2 e- ® H2O2(aq) + 2 H2(g)
e.
2 H2O(ª) ® 2 H2(g) + O2(g) + 4 e-
 

 98. 
Write a balanced half-reaction for the reduction of NO3-(aq) to NO(g) in an acidic solution.
a.
NO3-(aq) + H+(aq) + e- ® NO(g) + HO2(aq)
b.
NO3-(aq) + 2 H+(aq) + e- ® NO(g) + 2 OH-(aq)
c.
NO3-(aq) + 3 e- ® NO(g) + 2 O2(g)
d.
NO3-(aq) + 4 H+(aq) + 3 e- ® NO(g) + 2 H2O(ª)
e.
2 HNO3(aq) + 6 e- ® NO(g) + H2(g) + 3 O2(g)
 

 99. 
Write a balanced chemical equation for the following reaction in an acidic solution.

Cr2O72-(aq) + Fe2+(aq) ® Cr3+(aq) + Fe3+(aq)
a.
Cr2O72-(aq) + Fe2+(aq) ® 2 Cr3+(aq) + Fe3+(aq)
b.
Cr2O72-(aq) + Fe2+(aq) + 7 H+(aq) ® 2 Cr3+(aq) + Fe3+(aq) + 7 OH-(aq)
c.
Cr2O72-(aq) + 6 Fe2+(aq) + 7 H+(aq) ® 2 Cr3+(aq) + 6 Fe3+(aq) + 7 OH-(aq)
d.
Cr2O72-(aq) + Fe2+(aq) + 14 H+(aq) ® 2 Cr3+(aq) + Fe3+(aq) + 7 H2O(ª)
e.
Cr2O72-(aq) + 6 Fe2+(aq) + 14 H+(aq) ® 6 Fe3+(aq) + 2 Cr3+(aq) + 7 H2O(ª)
 

 100. 
All of the following statements concerning voltaic cells are true EXCEPT
a.
the two half-cells are connected by a salt bridge.
b.
electrons flow from the anode to the cathode.
c.
oxidation occurs at the cathode.
d.
voltaic cells can be used as a source of energy.
e.
a voltaic cell consists of two-half cells.
 

 101. 
What is the correct cell notation for the reaction below?

Cu2+(aq) + Pb(s) ® Cu(s) + Pb2+(aq)
a.
Pb | Pb2+(aq) || Cu2+(aq) | Cu
b.
Pb | Cu2+(aq) || Pb2+(aq) | Cu
c.
Pb | Cu(s) || Pb2+(aq) | Cu2+
d.
Cu | Pb2+(aq) || Cu2+(aq) | Pb
e.
Cu | Cu2+(aq) || Pb2+(aq) | Pb
 

 102. 
Write a balanced chemical equation for the overall reaction represented by the cell notation below.

Pt | H2(g) | H+(aq) | Cl-(aq) | Cl2(g) | Pt
a.
2 H+(aq) + 2 Cl-(aq) ® H2(g) + Cl2(g)
b.
Pt + 2 H+(aq) + 2 Cl-(aq) ® H2(g) + Cl2(g) + Pt
c.
2 Cl2(g) + 4 H+(aq) ® PtCl4(aq) + 2 H2(g)
d.
Cl2(g) + H2(g) ® 2 Cl-(aq) + 2 H+(aq)
e.
Cl2(g) + 2 H+(aq) ® 2 Cl-(aq) + H2(g)
 

 103. 
Consider the following half-reactions:

Fe3+(aq) + e- ® Fe2+(aq)
Eº = +0.77 V
Sn2+(aq) + 2 e- ® Sn(s)
Eº = -0.14 V
Fe2+(aq) + 2 e- ® Fe(s)
Eº = -0.44 V
Al3+(aq) + 3 e- ® Al(s)
Eº = -1.66 V
Mg2+(aq) + 2 e- ® Mg(s)
Eº = -2.37 V

Which of the above metals or metal ions are able to oxidize Al(s)?
a.
Fe3+ and Sn2+
b.
Fe3+, Sn2+, and Fe2+
c.
Fe2+, Sn, and Fe
d.
Mg and Mg2+
e.
Mg2+ only
 

 104. 
Given the following two half-reactions, determine which overall reaction is spontaneous and calculate the cell potential.

Mg2+(aq) + 2 e- ® Mg(s)
Eº = -2.37 V
Ni2+(aq) + 2 e- ® Ni(s)
Eº = -0.25 V
a.
Mg2+(aq) + Ni(s) ® Mg(s) + Ni2+(aq)          E1212finals05_files/i1050000.jpg = +2.12 V
b.
Mg2+(aq) + Ni(s) ® Mg(s) + Ni2+(aq)          E1212finals05_files/i1050001.jpg = -2.62 V
c.
Mg2+(aq) + Ni2+(aq) ® Mg(s) + Ni(s)          E1212finals05_files/i1050002.jpg = +2.62 V
d.
Mg(s) + Ni2+(aq) ® Ni(s) + Mg2+(aq)          E1212finals05_files/i1050003.jpg = +2.12 V
e.
Mg2+(aq) + Ni2+(aq) ® Ni(s) + Mg(s)          E1212finals05_files/i1050004.jpg = -2.12 V
 

 105. 
Calculate E1212finals05_files/i1060000.jpg for the following electrochemical cell:

Pt | H2(g) | H+(aq) || Pb2+(aq) | PbSO4(s) | Pb

given the following standard reduction potentials.

2 H+(aq) + 2 e- ® H2(g)
Eº = 0.000 V
PbSO4(s) + 2 e- ® Pb(s) + SO 42-(aq)
Eº = -0.356 V
a.
-0.712 V
b.
-0.356 V
c.
-0.178 V
d.
+0.356 V
e.
+0.712 V
 

 106. 
Which one of the changes below will increase the potential of the following electrochemical cell?

Pt | Sn4+(aq, 1.0 M), Sn2+(aq, 1.0 M) || Cu2+(aq, 0.200 M) | Cu
a.
Switching from a platinum to a graphite anode.
b.
Increasing the size of the cathode.
c.
Decreasing the concentration of Cu2+.
d.
Increasing the concentration of Sn2+.
e.
Increasing the temperature of the cell.
 

 107. 
Calculate 1212finals05_files/i1080000.jpg for the disproportionation of Cu+,

2 Cu+(aq) ® Cu2+(aq) + Cu(s)

given the following standard reduction potentials.

Cu+(aq) + e- ® Cu(s)
Eº = +0.518 V
Cu2+(aq) + 2 e- ® Cu(s)
Eº = +0.337 V
a.
-1180 kJ
b.
-175 kJ
c.
-165 kJ
d.
-56.8 kJ
e.
-34.9 kJ
 

 108. 
If 1212finals05_files/i1090000.jpg for the following reaction is -1.73 ´ 103 J, calculate 1212finals05_files/i1090001.jpg.

Cr2O72-(aq) + 2 Al(s) + 14 H+(aq) ® 2 Cr3+(aq) + 2 Al3+(aq) + 7 H2O(ª)
a.
+1.49 V
b.
+2.18 V
c.
+2.99 V
d.
+4.48 V
e.
+5.98 V
 

 109. 
What is the equilibrium constant for the following reaction at 25ºC?

Ni(s) + Cd2+(s) ® Ni2+(aq) + Cd(s)         1212finals05_files/i1100000.jpg = -0.15 V
a.
2.1 ´ 10-12
b.
8.4 ´ 10-6
c.
1.0 ´ 10-1
d.
1.2 ´ 101
e.
1.2 ´ 105
 

 110. 
What charge, in coulombs, is required to deposit 0.205 g Ag(s) from a solution of Ag+(aq)?
a.
2.29 C
b.
54.6 C
c.
103 C
d.
183 C
e.
197 C
 

 111. 
The least penetrating type of radiation can be stopped by clothing or a few pieces of paper. This type of radiation is a(n)
a.
alpha particle.
b.
beta particle.
c.
gamma particle.
d.
positron.
e.
cathode ray.
 

 112. 
Which one of the following symbols is used to represent gamma ray emission?
a.
1212finals05_files/i1130000.jpg
b.
1212finals05_files/i1130001.jpg
c.
1212finals05_files/i1130002.jpg
d.
1212finals05_files/i1130003.jpg
e.
1212finals05_files/i1130004.jpg
 

 113. 
Which of the following reactions is an example of beta particle emission?
a.
1212finals05_files/i1140000.jpg
b.
1212finals05_files/i1140001.jpg
c.
1212finals05_files/i1140002.jpg
d.
1212finals05_files/i1140003.jpg
e.
1212finals05_files/i1140004.jpg
 

 114. 
The atomic number of a nucleus that undergoes electron capture will
a.
decrease by two units.
b.
decrease by one unit.
c.
remain the same.
d.
increase by one unit.
e.
increase by two units.
 

 115. 
The mass number of a nucleus that emits an alpha particle will
a.
decrease by four units.
b.
decrease by two units.
c.
remain the same.
d.
increase by two units.
e.
increase by two units.
 

 116. 
What particle is produced in the following reaction?

1212finals05_files/i1170000.jpg + 1212finals05_files/i1170001.jpg ® 1212finals05_files/i1170002.jpg + _____
a.
1212finals05_files/i1170003.jpg
b.
1212finals05_files/i1170004.jpg
c.
1212finals05_files/i1170005.jpg
d.
1212finals05_files/i1170006.jpg
e.
1212finals05_files/i1170007.jpg
 

 117. 
Strontium-90 has a half-life of 28.1 years. Starting with 3.2 mg of this isotope, how much would remain after 112.4 years?
a.
0.1 mg
b.
0.2 mg
c.
0.4 mg
d.
0.8 mg
e.
1.6 mg
 

 118. 
What do scientists call the sequence of rapidly occurring reactions that results when a nuclear fission reaction produces enough neutrons to produce more fission reactions?
a.
nuclear fusion
b.
nuclear fission
c.
chain reaction
d.
neutron emission
e.
binding energy
 

 119. 
Enriched uranium is uranium that has a greater proportion of
a.
lead-207.
b.
radium-226.
c.
uranium-235.
d.
uranium-238.
e.
plutonium-248.
 

 120. 
What role do the cadmium control rods play in a fission reactor?
a.
They emit electrons which initiate the fission reaction.
b.
The cadmium combines with spent uranium fuel to produce a non-radioactive product.
c.
They focus the neutrons toward the center of the reactor.
d.
The cadmium acts as a catalyst, enabling fission to occur at lower temperatures.
e.
They control the rate of fission by absorbing neutrons.
 

 121. 
All of the following statements regarding isomers are correct EXCEPT
a.
optical isomers have non-superimposable mirror images.
b.
there are two types of stereoisomers, geometric and optical isomers.
c.
enantiomers are pairs of non-superimposable molecules.
d.
enantiomers have different physical properties, such as melting point and color.
e.
molecules with non-superimposable mirror images are said to be chiral.
 

 122. 
How many structural isomers exist for C5H12?
a.
1
b.
2
c.
3
d.
4
e.
8
 

 123. 
Which of the following (non-cyclic) hydrocarbons has at least two p bonds?
a.
C4H8
b.
C10H20
c.
C8H18
d.
C5H12
e.
C3H4
 

 124. 
What is the name of the following compound?

1212finals05_files/i1250000.jpg
a.
4,5-dihexane
b.
2,3-diethylhexane
c.
4,5-dimethane
d.
2,3-dimethylhexane
e.
4,5-dimethylhexane
 

 125. 
What is the name of the following compound?

1212finals05_files/i1260000.jpg
a.
3-methyl-5-ethylheptane
b.
3,5-diethylhexane
c.
2-methyl-4-ethylpentane
d.
2,4-diethylhexane
e.
5-ethyl-3-methylheptane
 

 126. 
What is the name of the following compound?

1212finals05_files/i1270000.jpg
a.
cis-4-propyl-3-butene
b.
ethyl-propylethene
c.
cis-ethyl-propylethene
d.
cis-3-heptene
e.
cis-5-ethyl-4-pentene
 

 127. 
What is the name of the following compound?

1212finals05_files/i1280000.jpg
a.
4-methyl-2-pentyne
b.
4,4-dimethylbutyne
c.
4,4-dimethyl-2-butyne
d.
2-methyl-3-pentyne
e.
2-methyle-3,4-pentadyne
 

 128. 
Which of the following compounds are aromatic?

1212finals05_files/i1290000.jpg
a.
3 only
b.
1 and 4
c.
2 only
d.
1, 2, and 4
e.
4 only
 

 129. 
How many isomers are possible for dichlorotoluene? Toluene is a benzene ring with a single methyl substituent.
a.
1
b.
2
c.
4
d.
6
e.
8
 

 130. 
What is the name of the following benzene derivative?

1212finals05_files/i1310000.jpg
a.
3-chlorobenzoic acid
b.
2-chlolobenzoic acid
c.
1-nitro-3-chlorobenzene
d.
1-carbonate-3-chlorobenzene
e.
3-chlorotoluene
 

 131. 
Which functional group does not contain an oxygen atom?
a.
alcohol
b.
amine
c.
amide
d.
ester
e.
ether
 

 132. 
The functional group RCOR' is characteristic of an ________.
a.
ester
b.
alcohol
c.
amine
d.
aldehyde
e.
amide
 

 133. 
The C=O linkage occurs in molecules with the following functional groups EXCEPT ________.
a.
esters
b.
ketones
c.
amines
d.
carboxylic acids
e.
aldehydes
 

 134. 
What is the product of the reaction of an aldehyde with potassium dichromate?
a.
ketone
b.
alcohol
c.
ester
d.
alkane
e.
carboxylic acid
 

 135. 
What class of compounds is responsible for many of the distinctive odors of artificial flavors and perfumes?
a.
esters
b.
ethers
c.
aldehydes
d.
amides
e.
amines
 

 136. 
What is the monomer of Teflon?
a.
CH2CH2
b.
CHFCHF
c.
CF2CH2
d.
CF2CF2
e.
CHFCF2
 

 137. 
All of the following statements concerning polymers are correct EXCEPT
a.
elastomers are materials that spring back to their original shape when stretched.
b.
polymers formed from two or more different monomers are called copolymers.
c.
thermoplastics can withstand very high temperatures without softening or melting.
d.
polystyrene is nonpolar and dissolves well in nonpolar solvents.
e.
a condensation reaction involves two different monomers, each with two different functional groups.
 

 138. 
Amino acids polymerize in condensation reactions that result in the formation of an amide linkage (or peptide bond. between amino acid molecules. What is a possible dipeptide formed in the reaction of glycine with phenylalanine?

1212finals05_files/i1390000.jpg
a.
Figure a
b.
Figure b
c.
Figure c
d.
Figure d
e.
none of the above
 

 139. 
Polyethylene
a.
is an example of a condensation polymer.
b.
reacts with methanol to form Dacron.
c.
contains no double bonds.
d.
contains equal numbers of cis and trans bonds.
e.
cannot form branched chains.
 

 140. 
Polypropylene is used in bottles, carpet, and films. It is produced by the addition reaction of propylene (propene). What is the structure of the polymer produced in this reaction?
1212finals05_files/i1410000.jpg
a.
Figure a
b.
Figure b
c.
Figure c
d.
Figure d
e.
Figure e
 



 
Submit          Reset Help