Use the following answers for questions 1 - 3.
(A) F1. Forms monatomic ions with 2¯ charge in solutions
(B) S
(C) Mg
(D) Ar
(E) Mn
2. Forms a compound having the formula KXO4
3. Forms oxides that are common air pollutants and that yield acidic solution in water
Use the following answers for questions 4 - 7.
(A) Hydrofluoric acid4. Is a good oxidizing agent
(B) Carbon dioxide
(C) Aluminum hydroxide
(D) Ammonia
(E) Hydrogen peroxide
5. Is used to etch glass chemically
6. Is used extensively for the production of fertilizers
7. Has amphoteric properties
Use the following answers for questions 8 - 9.
(A) A network solid with covalent bonding8. Solid ethyl alcohol, C2H5OH
(B) A molecular solid with zero dipole moment
(C) A molecular solid with hydrogen bonding
(D) An ionic solid
(E) A metallic solid
9. Silicon dioxide, SiO2
Use the following answers for questions 10 - 13.
(A) CO32¯Assume that you have an "unknown" consisting of an aqueous solution of a salt that contains one of the ions listed above. Which ions must be absent on the basis of each of the following observations of the "unknown"?
(B) Cr2O72¯
(C) NH4+
(D) Ba2+
(E) Al3+
10. The solution is colorless
11. The solution gives no apparent reaction with dilute hydrochloric acid.
12. No odor can be detected when a sample of the solution is added drop by drop to a warm solution of sodium hydroxide.
13. No precipitate is formed when a dilute solution of H2SO4 is added to a sample of the solution.
Questions 14-17
2Ag+ + Cd(s) ---> 2 Ag(s) + Cd2+
(A) Voltage increases.Which of the above occurs for each of the following circumstances?
(B) Voltage decreases but remains at zero.
(C) Voltage becomes zero and remains at zero.
(D) No change in voltage occures.
(E) Direction of voltage change cannot be predicted without additional information.
14. A 50-milliliter sample of a 2-molar Cd(NO3)2 solution is added to the left beaker.
15. The silver electrode is made larger.
16. The salt bridge is replaced by a platinum wire
17. Current is allowed to flow for 5 minutes
18.
| Hydrogen Halide | Normal Boiling Point, °C |
| HF | +19 |
| HCl | - 85 |
| HBr | - 67 |
| HI | - 35 |
The liquefied hydrogen halides have the normal boiling points given above. The relatively high boiling point of HF can be correctly explained by which of the followng?
(A) HF gas is more ideal.19. Which of the following represents a pair of isotopes?
(B) HF is the strongest acid.
(C) HF molecules have a smaller dipole moment.
(D) HF is much less soluble in water.
(E) HF molecules tend to form hydrogen bonds.
| Atomic
Number |
Mass
Number |
||
| (A) | I.
II. |
6
7 |
14
14 |
| (B) | I.
II. |
6
14 |
7
14 |
| (C) | I.
II. |
6
14 |
14
28 |
| (D) | I.
II. |
7
7 |
13
14 |
| (E) | I.
II. |
8
16 |
16
20 |
20. .....Mg(s) + .....NO3¯(aq) +.....H+(aq)
--->......Mg2+(aq) + ....NH When the skeleton equation above is balanced and all coefficients reduced
to their lowest whole-number terms. what is the coeficient for H+
?
Atoms of an element, X, have the electronic configuration shown above.
The compound most likely formed with magnesium, Mg, is
H3AsO4 + 3I¯ + 2 H3O+
---> H3AsO3 + I>3¯ + H2O The oxidation of iodide ions by arsenic acid in acidic aqueous solution
occurs according to the stoichiometry shown above. The experimental rate
law of the reaction is:
Rate = k [H3AsO4] [I¯] [H3O+] 25. What is the order of the reaction with respect to I¯?
When the concentration of substance B in the reaction above is doubled,
all other factors being held constant, it is found that the rate of the
reaction remains unchanged. The most probable explanation for this observation
is that
If the equilibrium constant for the reaction above is 3.7 x 1015,
which of the following correctly describes the standard voltage, E°,
and the standard free energy change, DG°,
for this reaction?
When the substances in the equation above are at equilibrium at pressure
P and temperature T, the equilibrium can be shifted to favor the products
by
DHf° H2O(l) = -
285.8 kJ / mole
DHf° CO2(g) = -
393.3 kJ / mole
What is the standard heat of formation of methane, DHf°
CH4(g), as calculated from the data above?
The reaction of silver metal and dilute nitric acid proceeds according
to the equation above. If 0.10 mole of powdered silver is added to 10.
milliliters of 6.0-molar nitric acid, the number of moles of NO gas that
can be formed is
57. For the reaction A(g) <===> B(g) + C(g), the equilibrium constant,
Kp, is 2 x 10¯4 at 25 °C. A mixture of the
three gases at 25 °C is placed in a reaction flask and the initial
pressures are PA = 2 atmosphere, PB = 0.5 atmosphere,
and PC = 1 atmosphere, At the instant of mixing, which of the
following is true for the reaction as written?
Volumes of NaOH Solution
On the basis of the information above, a buffer with a pH = 9 can best
be made by using
Gaseous atoms of which of the elements above are paramagnetic?
Consider the equilibrium above. Which of the following changes will
increase the concentration of HgI42¯?
(A) (B) (C) (D) (E) 78. When the actual gas volume is greater then the volume predicted
by the ideal gas law, the explanation lies in the fact that the ideal gas
law does NOT include a factor for molecular.
In a titration experiment based on the equation above, 25.0 milliliters
of an acidified Fe2+ solution requires 14.0 milliliters of standard
0.050-molar MnO4¯ solution to reach the equivalence point.
The concentration of Fe2+ in the original soluiton is
Nitramide, N2H2O2, decomposes slowly
in aqueous solution. This decomposition is believed to occur according
to the reaction mechanism above. The rate law for the decomposition of
nitramide that is consistent with this mechanism is given by which of the
following?
At constant temperature, DH, the change in
enthalpy for the reaction above is approximately equal to
(A) 4
21. When a sample of oxygen gas in a closed container of constant volume
is heated until its absolute temperature is doubled, which of the following
is also doubled?
(B) 6
(C) 8
(D) 9
(E) 10(A) The density of the gas
22. 1s2 2s22p6 3s23p3
(B) The pressure of the gas
(C) The average velocity of the gas molecules
(D) The number of molecules per cm3
(E) The potential energy of the molecules(A) MgX
23. The density of an unknown gas is 4.20 grams per liter at 3.00 atmospheres
pressure and 127 °C. What is the molecular weight of this gas? (R =
0.0821 liter-atm / mole-K)
(B) Mg2X
(C) MgX2
(D) MgX3
(E) Mg3X2(A) 14.6
24. The formula for potassium hexacyanoferrate(II) is
(B) 46.0
(C) 88.0
(D) 94.1
(E) 138(A) K4[Fe(CN)6]
Questions 25-26
(B) K3[Fe(CN)6]
(C) K2[Pt(CN)4]
(D) K2[Pt(CN)6]
(E) KCN(A) 1
26. According to the rate law for the reaction, an increase in the concentration
of hydronium ion has what effect on this reaction?
(B) 2
(C) 3
(D) 5
e. 6(A) The rate of reaction increases.
27. The critical temperature of a substance is the
(B) The rate of reaction decreases.
(C) The value of the equilibrium constant increases.
(D) The value of the equilibrium constant decreases.
(E) Neither the rate nor the value of the equilibrium constant is changed.(A) temperature at which the vapor pressure of the liquid is
equal to the external pressure
28. 2 A(g) + B(g) <===> 2 C(g)
(B) temperature at which the vapor pressure of the liquid is equal
to 760 mm Hg
(C) temperature at which the solid, liquid, and vapor phases are all
in equilibrium
(D) Temperature at which liquid and vapor phases are in equilibrium
at I atmosphere
(E) lowest temperature above which a substance cnnot be liquified at
any applied pressure(A) the order of the reaction with respect to substance B is
1
29. Cu(s) + 2 Ag+ ---> Cu2+ + 2 Ag(s)
(B) substance B is not involved in any of the steps in the mechanism
of the reaction
(C) substance B is not involved in the rate-determining step of the
mechanism, but is involved in subsequent steps
(D) substance B is probably a catalyst, and as such, its effect on
the rate of the reaction does not depend on its concentration
(E) the reactant with the smallest coefficient in the balanced equation
generally has little or no effecton the rate of the reaction(A) E° is positive and DG°
is negative.
30. When 84-Po-214 decays, the emission consists consecutively of an alpha
particle, then two beta particles, and finally another alpha particle.
The resulting stable nucleus is
(B) E° is negative and DG° is positive.
(C) E° and DG° are both positive.
(D) E° and DG° are both negative.
(E) E° and DG° are both zero(A) 83-Bi-206
31. A 0.1-molar solution of which of the following ions is orange?
(B) 83-Bi-210
(C) 82-Pb-206
(D) 82-Pb-208
(E) 81-Tl-210(A) Fe(H2O)42+
32. The net ionic equation for the reaction between silver carbonate and
hydrochloric acid is
(B) Cu(NH3)42+
(C) Zn(OH)42¯
(D) Zn(NH3)42+
(E) Cr2O72¯(A) Ag2CO3(s) + 2 H+ + 2 Cl¯
---> 2 AgCl(s) + H2O + CO(g)
33. The pH of 0.1-molar ammonia is approximately
(B) 2 Ag+ + CO32¯ + 2 H+
+ 2 Cl¯ ---> 2 AgCl(s) + H2O + CO2(g)
(C) CO32¯ + 2 H+ ---> H2O
+ CO2(g)
(D) Ag+ + Cl¯ ---> AgCl(s)
(E) Ag2CO3(s) + 2 H+ ---> 2Ag+
+ H2CO3(A) 1
34. ...CrO2¯ + ...OH¯ ---> ... CrO42¯
+ ... H2O + ... e¯ When the equation for the half-reaction
above is balanced, what is the ratio of the coefficients OH¯ / CrO2¯
?
(B) 4
(C) 7
(D) 11
(E) 14(A) 1:1
35. The addition of an oxidizing agent such as chlorine water to a clear
solution of an unknown compound results in the appearance of a brown color.
When this solution is shaken with the organic solvent, methylene dichloride,
the organic solvent layer turns purple. The unknown compound probably contains
(B) 2:1
(C) 3:1
(D) 4:1
(E) 5:1(A) K+
36. CuO(s) + H2(g) <===> Cu(s) + H2O(g);
DH
= - 2.0 kilojoules
(B) Br¯
(C) NO3¯
(D) I¯
(E) Co2+(A) increasing the pressure by means of a moving piston at
constant T
37. The molality of the glucose in a 1.0-molar glucose solution can be
obtained by using which of the following?
(B) increasing the pressure by adding an inert gas such as nitrogen
(C) decreasing the temperature
(D) allowing some gases to escape at constant P and T
(E) adding a catalyst(A) Volume of the solution
38. The radioactive decay of 6-C-14 to 7-N-14 occurs by the process of
(B) Temperature of the solution
(C) Solubility of glucose in water
(D) Degree of dissociation of glucose
(E) Density of the solution(A) beta particle emission
39. Equal masses of three different ideal gases, X, Y, and Z, are mixed
in a sealed rigid container. If the temperature of the system remains constant,
which of the following statements about the partial pressure of gas X is
correct?
(B) alpha particle emission
(C) positron emission
(D) electron capture
(E) neutron capture(A) It is equal to 1/3 the total pressure
40. The geometry of the SO3 molecule is best described as
(B) It depends on the intermolecular forces of attraction between molecules
of X, Y, and Z.
(C) It depends on the relative molecular masses of X, Y, and Z.
(D) It depends on the average distance traveled between molecular collisions.
(E) It can be calculated with knowledge only of the volume of the container.(A) trigonal planar
41. Which of the following molecules has the shortest bond length?
(B) trigonal pyramidal
(C) square pyramidal
(D) bent
(E) tetrahedral(A) N2
42. Metallic copper is heated strongly with concentrated sulfuric acid.
The products of this reaction are
(B) O2
(C) Cl2
(D) Br2
(E) I2(A) CuSO4(s) and H2(g) only
43. The elements in which of the following have most nearly the same atomic
radius?
(B) Cu2+, SO2(g), and H2O
(C) Cu2+, H2(g), and H2O
(D) CuSO4(s), H2(g), and SO2(g)
(E) Cu2+, SO3(g), and H2O(A) Be, B, C, N
44. What number of moles of O2 is needed to produce 14.2 grams
of P4O10 from P? (Molecular weight P4O10
= 284)
(B) Ne, Ar, Kr, Xe
(C) Mg, Ca, Sr, Ba
(D) C, P, Se, I
(E) Cr, Mn, Fe, Co(A) 0.0500 mole
45. The alkenes are compounds of carbon and hydrogen with the general formula
CnH2n. If 0.561 gram of any alkene is burned in excess
oxygen, what number of moles of H2O is formed?
(B) 0.0625 mole
(C) 0.125 mole
(D) 0.250 mole
(E) 0.500 mole(A) 0.0400 mole
46. If 0.060 faraday is passed through an electrolytic cell containing
a solution of In3+ ions, the maximum number of moles of In that
could be deposited at the cathode is
(B) 0.0600 mole
(C) 0.0800 mole
(D) 0.400 mole
(E) 0.800 mole(A) 0.010 mole
47. CH4(g) + 2 O2(g) ---> CO2(g) + 2 H2O(l);
D = - 889.1 kJ
(B) 0.020 mole
(C) 0.030 mole
(D) 0.060 mole
(E) 0.18 mole(A) -210.0 kJ/mole
48. Which of the following ions is the strongest Lewis acid?
(B) -107.5 kJ/mole
(C) -75.8 kJ/mole
(D) 75.8 kJ/mole
(E) 210.0 kJ/mole(A) Na+
49. Each of the following can act as both a Brönsted acid and a Brönsted
base EXCEPT
(B) Cl¯
(C) CH3COO¯
(D) Mg2+
(E) Al3+(A) HCO3¯
50. Two flexible containers for gases are at the same temperature and pressure.
One holds 0.50 gram of hydrogen and the other holds 8.0 grams of oxygen.
Which of the following statements regarding these gas samples is FALSE?
(B) H2PO4¯
(C) NH4+
(D) H2O
(E) HS¯(A) The volume of the hydrogen container is the same as the
volume of the oxygen container.
51. Pi bonding occurs in each of the following species EXCEPT
(B) The number of molecules in the hydrogen container is the same as
the number of molecules in the oxygen container.
(C) The density of the hydrogen sample is less than that of the oxygen
sample.
(D) The average kinetic energy of the hydrogen molecules is the same
as the average kinetic energy of the oxygen molecules.
(E) The average speed of the hydrogen molecules is the same as the
average speed of the oxygen molecules.(A) CO2
52. 3 Ag(s) + 4 HNO3 <===> 3 AgNO3 + NO(g) + 2
H2O
(B) C2H4
(C) CN¯
(D) C6H6
(E) CH4(A) 0.015 mole
53. Which, if any, of the following species is in the greatest concentration
in a 0.100-molar solution of H2SO4 in water?
(B) 0.020 mole
(C) 0.030 mole
(D) 0.045 mole
(E) 0.090 mole(A) H2SO4 molecules
54. Which of the following statements is always true about the phase diagram
of any one-component system?
(B) H3O+ ions
(C) HSO4¯ ions
(D) SO42¯ ions
(E) All species are in equilibrium and therefore have the same concentrations.(A) The slope of the curve representing equilibrium between
the vapor and liquid phases is positive.
55. At 20. °C, the vapor pressure of toluene is 22 millimeters of mercury
and that of benzene is 75 millimeters of mercury. An ideal solution, equimolar
in toluene and benzene, is prepared. At 20. °C, what is the mole fraction
of benzene in the vapor in equilibrium with this solution?
(B) The slope of the curve representing equilibrium between the liquid
and solid phases is negative.
(C) The slope of the curve representing equilibrium between the liquid
and solid phases is positive.
(D) the temperature at the triple point is greater than the normal
freezing point.
(E) The pressure at the triple point is greater than 1 atmosphere.(A) 0.23
56. A cube of ice is added to some hot water in a rigid, insulated container,
which is then sealed. There is no heat exchange with the surroundings.
What has happened to the total energy and the total entropy when the system
reaches equilibrium?
(B) 0.29
(C) 0.50
(D) 0.77
(E) 0.83
Energy
Entropy
(A)
Remains constant
Remains constant
(B)
Remains constant
Decreases
(C)
Remains constant
Increases
(D)
Decreases
Increases
(E)
Increases
Decreases
(A) DG < 0
58. Which of the following represents the ground state electron configuration
for the Mn3+ ion? (Atomic number Mn = 25)
(B) DG > 0
(C) DS = 0
(D) DG° = 0
(E) DG° < 0(A) 1s2 2s22p6 3s23p63d4
59. When 70. milliliter of 3.0-molar Na2CO3 is added
to 30. milliliters of 1.0-molar NaHCO3 the resulting concentration
of Na+ is
(B) 1s2 2s22p6 3s23p63d5
4s2
(C) 1s2 2s22p6 3s23p63d2
4s2
(D) 1s2 2s22p6 3s23p63d8
4s2
(E) 1s2 2s22p6 3s23p63d3
4s1(A) 2.0 M
60. Which of the following has a zero dipole moment?
(B) 2.4 M
(C) 4.0 M
(D) 4.5 M
(E) 7.0 M(A) HCN
61. When a solution of potassium dichromate is added to an acidified solution
of iron(II) sulfate, the products of the reaction are
(B) NH3
(C) SO2
(D) NO2
(E) PF5(A) FeCr2O7(s) and H2O
62. A student pipetted five 25.00-milliliter samples of hydrochloric acid
and transferred each sample to an Erlenmeyer flask, diluted it with distilled
water, and added a few drops of phenolphthalein to each. Each sample was
then titrated with a sodium hydroxide solution to the appearance of the
first permanent faint pink color. The following results were obtained.
(B) FeCrO4(s) and H2O
(C) Fe3+, CrO42¯, and H2O
(D) Fe3+, Cr3+, and H2O
(E) Fe2(SO4)3(s), Cr3+
and H2OFirst Sample..................35.22 mL
Which of the following is the most probable explanation for the variation
in the student's results?
Second Sample..............36.14 mL
Third Sample.................36.13 mL
Fourth Sample..............36.15 mL
Fifth Sample..................36.12 mL(A) The burette was not rinsed with NaOH solution.
63.
(B) The student misread a 5 for a 6 on the burette when the first sample
was titrated.
(C) A different amount of water was added to the first sample.
(D) The pipette was not rinsed with the HCI solution.
(E) The student added too little indicator to the first sample.
Acid
Acid Dissociation
Constant, Ka
H3PO4
7 x 10¯3
H2PO4¯
8 x 10¯8
HPO42¯
5 x 10¯13
(A) pure NaH2PO4
64. The net ionic equation for the reaction that occurs during the titration
of nitrous aicd with sodium hydroxide is
(B) H3PO4 + H2PO4¯
(C) H2PO4¯ + PO43¯
(D) H2PO4¯ + HPO42¯
(E) HPO42¯ + PO43¯(A) HNO2 + Na+ + OH¯ ---> NaNO2
+ H2O
65. Which of the following species CANNOT function as an oxidizing agent?
(B) HNO2 + NaOH ---> Na+ + NO2¯
+ H2O
(C) H+ + OH¯ --->H2O
(D) HNO2 + H2O ---> NO2¯ + H3O+
(E) HNO2 + OH¯ ---> NO2¯ + H2O(A) Cr2O72¯
66. Ca, V, Co, Zn, As
(B) MnO4¯
(C) NO3¯
(D) S
(E) I¯(A) Ca and As only
67. A student wishes to prepare 2.00 liters of 0.100-molar KIO3
(molecular weight 214). The proper procedure is to weigh out
(B) Zn and As only
(C) Ca, V, and Co only
(D) V, Co, and As only
(E) V, Co, and Zn only(A) 42.8 grams of KIO3 and add 2.00 kilograms of
H2O
68. A 20.0-milliliter sample of 0.200-molar K2CO3
solution is added to 30.0 milliliters of 0.400-molar Ba(NO3)2
solution. Barium carbonate precipitates. The concentration of barium ion,
Ba2+, in solution after reaction is
(B) 42.8 grams of KIO3 and add H2O until the
final homogeneous solution has a volume of 2.00 liters
(C) 21.4 grams of KIO3 and add H2O until the
final homogeneous solution has a volume of 2.00 liters
(D) 42.8 grams of KIO3 and add 2.00 liters of H2O
(E) 21.4 grams fo KIO3 and add 2.00 liters of H2O(A) 0.150 M
69. What is the mole fraction of ethanol, C2H5OH,
in an aqueous solution in which the ethanol concentration is 4.6 molal?
(B) 0.160 M
(C) 0.200 M
(D) 0.240 M
(E) 0.267 M(A) 0.0046
70. One of the outermost electrons in a strontium atom in the ground state
can be described by which of the following sets of four quantum numbers?
(B) 0.076
(C) 0.083
(D) 0.20
(E) 0.72(A) 5, 2, 0, 1/2
71. Which of the following reactions does NOT proceed significantly to
the right in aqueous solutions?
(B) 5, 1, 1, 1/2
(C) 5, 1, 0, 1/2
(D) 5, 0, 1, 1/2
(E) 5, 0, 0, 1/2(A) H3O+ + OH¯ ---> 2 H2O
72. A compound is heated to produce a gas whose molecular weight is to
be determined. The gas is collected by displacing water in a water-filled
flask inverted in a trough of water. Which of the following is necessary
to calculate the molecular weight of the gas, but does NOT need to be measured
during the experiment?
(B) HCN + OH¯ ---> H2O + CN¯
(C) Cu(H2O)42+ + 4 NH3
---> Cu(NH3)42++ + 4H2O
(D) H2SO4 + H2O ---> H3O+
+ HSO4¯
(E) H2O + HSO4¯ ---> H2SO4
+ OH¯(A) Mass of the compound used in the experiment
73. A 27.0-gram sample of an unknown hydrocarbon was burned in excess oxygen
to form 88.0 grams of carbon dioxide and 27.0 grams of water. What is a
possible molecular formula of the hydrocarbon?
(B) Temperature of the water in the trough
(C) Vapor pressure of the water
(D) Barometric pressure
(E) Volume of water displaced from the flask(A) CH4
74. How many moles of NaF must be dissolved in 1.00 liter of a saturated
solution of PbF2 at 25 °C to reduce the [Pb2+]
to 1 x 10¯6 molar? (Ksp of PbF2 at
25 °C = 4.0 x 10¯8)
(B) C2H2
(C) C4H3
(D) C4H6
(E) C4H10(A) 0.020 mole
75. If the acid dissociation constant, Ka, for an acid HA is
8 x 10¯4 at 25 °C, what percent of the acid is dissociated
in a 0.50-molar solution of HA at 25 °C?
(B) 0.040 mole
(C) 0.10 mole
(D) 0.20 mole
(E) 0.40 mole(A) 0.08%
76. HgO(s) + 4 I¯ + H2O <===> HgI42¯
+ 2 OH¯; DH < 0
(B) 0.2%
(C) 1%
(D) 2%
(E) 4%(A) Increasing the concentration of OH¯
77. Which of the following compounds exhibits optical isomerism?
(B) Adding 6 M HNO3
(C) Increasing the mass of HgO present
(D) Increasing the temperature
(E) Adding a catalyst
(A) volume
79. 5 Fe2+ + MnO4¯ + 8 H+ <===>
5 Fe3+ + Mn2+ + 4 H2O
(B) mass
(C) velocity
(D) attractions
(E) shape(A) 0.0010 M
80. For which of the following molecules are resonance structures necessary
to describe the bonding satisfactorily?
(B) 0.0056 M
(C) 0.028 M
(D) 0.090 M
(E) 0.14 M(A) H2S
81. What is the net ionic equation for the reaction that occurs when aqueous
copper(II) sulfate is added to excess 6-molar ammonia?
(B) SO2
(C) CO2
(D) OF2
(E) PF3(A) Cu2+ + SO42¯ + 2
NH4+ + 2 OH¯ ---> (NH4)2SO4
+ Cu(OH)2
82.
(B) Cu2+ + 4 NH3 + 4 H2O --> Cu(OH)42¯
+ 4 NH4+
(C) Cu2+ + 2 NH3 + 2 H2O --> Cu(OH)2
+ 2 NH4+
(D) Cu2+ + 4 NH3 --> Cu(NH3)42+
(E) Cu2+ + 2 NH3 + H2O --> CuO + 2
NH4+
Step 1) N2H2O2 <===>
N2HO2¯ + H+
(fast equilibrium)
Step 2) N2HO2¯ ---> N2O + OH¯
(slow)
Step 3) H+ + OH¯ ---> H2O
(fast)
(A) Rate = k [N2H2O2]
83. NH3(g) + 2 CH4(g) + 5/2 O2(g) <===>
H2NCH2COOH(s) + 3 H2O(l)
(B) Rate = k [N2H2O2] [H+]
(C) Rate = (k [N2H2O2]) / [H+]
(D) Rate = (k [N2H2O2]) / [N2HO2¯]
(E) Rate = k [N2H2O2] [OH¯](A) DE - (11/2)RT
84. Which of the following aqueous solutions has the highest boiling point?
(B) DE - (7/2)RT
(C) DE + RT
(D) DE + (7/2)RT
(E) DE (11/2)RT(A) 0.10 M potassium sulfate, K2SO4
85. A sample of 9.00 grams of aluminum metal is added to an excess of hydrochloric
acid. The volume of hydrogen gas produced at standard temperature and pressure
is
(B) 0.10 M hydrochloric acid, HCl
(C) 0.10 M ammonium nitrate, NH4NO3
(D) 0.10 M magnesium sulfalte, MgSO4
(E) 0.20 M sucrose, C12H22O11(A) 22.4 liters
(B) 11.2 liters
(C) 7.46 liters
(D) 5.60 liters
(E) 3.74 liters
Educational Testing Service. All rights reserved.