1
The density of octane is 0.703 g/mL. What mass (in g) will a 1.964 gallon sample of octane have?
2
Classify the properties as extensive or intensive.
Mass extensive - intensive
Density extensive - intensive
Color extensive - intensive
Volume extensive - intensive
Total energy extensive - intensive
Temperature extensive - intensive
Melting point extensive - intensive
3
For each set select the most abundant isotope or whether it cannot be determined.
Boron-10 and boron-11
A. boron-11
B. boron-10
C. can not be determined
4
Nitrogen has two isotopes one of which is nitrogen-14 with a percent abundance of 99.634% and a mass of 14.003074 amu. What is the mass of nitrogen-15?
5
Give the mass number for the species described. Hydrogen with no neutrons
6
How many electrons are in the species listed? Chromium with a 3+ charge
7
How many mol of carbon are in 33.1 g of carbon tetrachloride?
8
What is the mass of oxygen in 6.42 g of iron(III) oxide?
9
What is the total sample size (in grams) for a sample of magensium nitrate which contains 3.66 g of oxygen?
10
What is the name of HClO3 (when this substance is in a water solution)?
11
What is the sum of the stoichiometric coefficients when the reaction is balanced to lowest common denominator?
Fe2O3(s) + CO(g) → Fe(s) + CO2(g)
12
How many moles of oxygen react when 0.631 mol of ethanol (CH3CH2OH) are combusted in oxygen to produce carbon dioxide and water?
13
What is the experimental yield (in grams) of the solid product when the percent yield is 98.1 % when 5.708 g of barium chloride reacts in solution with excess sodium phosphate?
BaCl2(aq) + Na3PO4(aq) → Ba3(PO4)2(s) + NaCl(aq) [unbalanced]
14
What is the percent yield of the solid product when 12.38 g of iron(III) nitrate reacts in solution with excess sodium phosphate and 5.336 g of the precipitate is experimentally obtained?
Fe(NO3)3(aq) + Na3PO4(aq) → FePO4(s) + NaNO3(aq) [unbalanced]
15
What is the limiting reactant when equal masses of iron(II) chloride and sodium phosphate react in solution?
A. iron(II) phosphate
B. sodium chloride
C. iron(II) chloride
D. sodium phosphate
E. This reaction does not occur
F. Cannot be determined without actual masses.C
16
In the reaction of bromine with potassium iodide to produce potassium bromide and iodine, what is reduced and what is the reducing agent?
A. bromine is reduced and potassium iodide is the reducing agent
B. bromine is reduced and bromine is the reducing agent
C. iodine is reduced and potassium iodide is the reducing agent
D. iodine is reduced and bromine is the reducing agent
E. potassium is reduced and potassium iodide is the reducing agent
F. potassium is reduced and bromine is the reducing agent
17
Which reactions are redox reactions?
A. iron(III) oxide reacting with carbon monoxide to form liquid iron and carbon dioxide
B. copper reacting with nitric acid to form nitrogen dioxide, water and copper(II) nitrate
C. copper(II) nitrate reacting with potassium sulfide to form the precipitate copper(II) sulfide and aqueous potassium nitrate
D. nitrous acid reacting with potassium hydroxide to form potassium nitrite and water
E. ammonia reacting with hydrochloric acid to form ammonium chloride
F. hydrogen and oxygen reacting to form water
18
What is the concentration (in M) of the chloride ion when 18.8 mL of a 0.709 M solution of barium chloride is combined with 17.2 mL of a 0.611 M solution of aluminum chloride? Assume the volumes are additive.
19
What is the concentration of the ammonium ion (in M) in a solution which contains 58.8 g ammonium sulfide in 584 mL of solution?
20
What volume (in mL) of water must be added to a 1.346 M solution of sodium chloride to make a 52.1 mL of a 0.51999 M solution? Assume the volumes are additive.
21
What is the experimental yield (in g of precipitate) when 19.7 mL of a 0.6 M solution of iron(III) chloride is combined with 15.7 mL of a 0.598 M solution of lead(II) nitrate at a 75.5% yield?
22
What is the theoretical yield (in g of precipitate) when 17.6 mL of a 0.564 M solution of iron(III) chloride is combined with 19 mL of a 0.608 M solution of lead(II) nitrate?
23
Under constant pressure, at what temperature (in K) will a balloon double in size when originally at 110.9oC?
24
What is the density (in g/L) of nitric oxide (NO) at 314 K and under 1.338 atm of pressure?
25
What is the molar mass of a gas which occupies 42.2 L at 87oC under 690 torr of pressure and has a mass of 23 grams?
26
When 48 L of nitric oxide reacts with 44.5 L of oxygen at 402 K under a constant pressure of 1.693 atm, what is the theoretical yield (in g) of nitrogen dioxide?
27
Which  substance would most behave as an ideal gas at STP?
A. N2
B. H2O
C. CH3OH
D. HF
28
Nitrogen and hydrogen react in the Haber process to form ammonia. All substances are in the gas phase. If 0.453 atm of nitrogen and 0.686 atm of hydrogen react, what is the partial pressure of ammonia (in mmHg) when this reaction goes 59.4 complete. The volume and temperature are constant.
29
What is the root mean square speed (in m/s) of nitrogen at 27.6oC?
30
When 10.33 g of neon is combined in a 21.58 L container at 84oC with 9.53 g of argon, what is the partial pressure (in mmHg) of argon?
31
What is the final temperature (in oC) of a 37.1 g sample of graphite (specific heat = 0.720 J/(g K)) which absorbs 9.49 kJ of heat when it warms from 18.51oC?
32
An 34.75 g sample of aluminum is placed on a 43.58 g sample of copper initially at 110.46oC. If the heat is only transferred between the metals (with no loss to the surroundings) and the final temperature of both metals is 47.69oC, what is the inital temperature (in oC) of aluminum?
33
How much heat (in kJ) is evolved (under standard conditions) when 205.36 g of copper reacts to form copper(II) oxide?
34
How much heat (in kJ) is needed when 62.15 g of water warms and boils from 54.76oC to 100oC?
35
What is recorded as the final temperature (in oC) on a constant pressure calorimeter if 12.284 g of potassium hydroxide is dissolved in 28.71 mL of water originally at 24.153oC?
36
What is the coefficient for nitrogen in the formation reaction for ammonia? Enter any fraction as a decimal.
37
What is the enthalpy of formation of butane (C4H10) if the enthalpy of combustion for butane is -2876.9 kJ/mol (water is produced as a liquid)? Use the appendix in your textbook, do not enter units, and answer with 3 significant digits.
38
In the photoelectric effect, above the threshhold frequency, the number of ejected electrons is proportional to
A. the intensity of the incident light.
B. the frequency of the incident light.
C. the speed of the incident light.
39
Which ion is paramagnetic in the ground state?
A. Fe3+
B. Al3+
C. S2-
D. Zn2+
E. Ag+
F. F-
40
Which set(s) of quantum numbers is/are not possible for a ground state electron in zinc?
A. (4, 1, 0, 1/2)
B. (4, 0, 0, 1/2)
C. (3, 2, -2, 1/2)
D. (2, 0, 0, 1/2)
E. (5, 0, 0, 1/2)
F. (4, 2, 2, 1/2)
41
How many values of l are possible when n = 4?
42
What is the energy (in J) of a photon when an electron relaxes from n = 4 to n = 2 in a hydrogen atom?
Answer with no units, to 2 significant digits and using exponential notion as "1.0x10-10" entered as "1.0x10(-10)"
43
What ion(s) is/are not isoelectronic with a neon atom?
A. the potassium ion
B. the sodium ion
C. the chloride ion
D. the oxide ion
E. the nitride ion
F. the calcium ion
44
What is the periodic trend for atomic radii?
A. decreasing right to left in a period, increasing bottom to top in a group
B. increasing right to left in a period, increasing bottom to top in a group
C. decreasing right to left in a period, decreasing bottom to top in a group
D. increasing right to left in a period, decreasing bottom to top in a group
45
What is the periodic trend for first ionization energy?
A. increasing right to left in a period, decreasing bottom to top in a group
B. increasing right to left in a period, increasing bottom to top in a group
C. decreasing right to left in a period, decreasing bottom to top in a group
D. decreasing right to left in a period, increasing bottom to top in a group
46
Which element exhibits the least metallic character?
A. Be
B. Ca
C. Mg
D. Ba
47
Using the equation in your textbook (9.2, p. 291) as an approximation, which ionic compound will have the greatest lattice energy?
A. LiF
B. LiCl
C. NaF
D. NaCl
48
How many lone pairs of electrons are on the central atom in xenon tetrafluoride?
49
How many resonance structures does the nitrite ion have?
50
What is the formal charge on nitrogen in the nitrite ion?
51
Using the table of bond enthalpies in your textbook, what is the change in enthalpy (in kJ) when 1.1 mol of HCN molecules are broken into atoms?
52
What is the carbon-oxygen bond length in the carbonate ion?
A. between C-O and C=O
B. two are C-O and one is C=O
C. all are C-O
D. all are C=O
E. all are longer than C-O
F. all are shorter than C=O
G. two are C=O and one is C-O
53
Which molecule has the greatest dipole moment?
A. HF
B. HCl
C. HBr
D. HI
54
How many pi bonds are in one molecule of acetylene, HCCH?
55
How many sigma bonds are in one molecule of dinitrogen monoxide?
56
Using a MO diagram, how many antibonding electrons are in one molecule of nitrogen
57
What is the hybridization on either central atom in acetylene, HCCH?
Enter your answer with no spaces and no superscripts, for example, sp2 is entered as "sp2".
58
What is the hybridization on the central atom in formaldehyde, COH2?
Enter your answer with no spaces and no superscripts, for example, sp2 is entered as "sp2".
59
What is the shape of iodine trichloride?
60
At higher elevations, what is the effect the pressure on the boiling point of a substance?
A. the boiling point is lowered because the external pressure is lower
B. the boiling point is lowered because the external pressure is higher
C. the boiling point is raised because the external pressure is lower
D. the boiling point is raised because the external pressure is higher
61
What type of bonding is present in a solid which is hard, has a high melting point, and is not conductive in the solid state?
A. covalent
B. ionic
C. metallic
D. molecular
62
What type(s) of intermolecular forces are present between hydrogen bromide and water?
A. dipole-dipole
B. dispersion
C. dipole-induced dipole
D. ion-induced dipole
E. ion-dipole
63
What type(s) of intermolecular forces are present in the pure molecular substance of acetic acid?
A. dispersion
B. ionic
C. dipole
D. hydrogen bonding
E. covalent bonding
64
The density of an aqueous solution of nitric acid is 1.62 g/mL and the concentration is 2.67 M. What is the concentration of this solution in m?
65
The density of an aqueous solution of sulfuric acid is 1.75 g/mL and the concentration is 2.06 M. What is the concentration of this solution in mole fraction?
66
What is the density (in g/cm3) of a fictious elemental solid which packs in a body-centered cubic unit cell with an edge length of 273 pm and a molar mass of 161 g/mol?
67
The vapor pressure of water at 45oC is 71.88 mmHg. What is the vapor pressure of a sugar (C12H22O11) solution made by dissolving 52.39 g of sugar in 90.92 g of water?
68
What is the freezing point of water made by dissolving 18.32 g of sodium chloride in 91.14 g of water? The freezing-point depression constant of water is 1.86 oC/m.
69
If the initial rate is 0.0835 M/s for a reaction with a rate law of rate = k[A]0[B], what is the value of the rate constant when the initial concentration of [A] is 0.0904 M and [B] is 0.0693 M?
70
For a first order decay of [A], if 496 mg remains of an initial sample of 1.4685 g after 510 min, what is the half life (in minutes)?
71
The decay of carbon-14 is first order with a half life is 6053 years. How much of 1.2835 g sample would remain after 8973 years?
72
If the rate constant for a reaction at 67.61 oC is 0.632 s-1 and the activation energy is 35.13 kJ/mol, what is the rate constant at 119.1oC?
73
For the reaction mechanism,
A + B → C + D (slow)
A + D → E + B (fast)
the rate determining step is
a. unimolecular.
b. bimolecular.
c. termolecular.
d. cannot be determined.
74
For the reaction mechanism,
A + B → C + D (slow)
A + D → E + B (fast)
what is the catalyst?
75
The reaction of A → products is second order. Therefore, plotting what versus time will result in a straight line?
a. [A]
b. ln [A]
c. 1/[A]
d. [A]2
76
For which reaction is KC = [CO2]?
(Note: For all equilibrium problems, the single direction arrow should be a double arrow representing an equilibrium.)
a. CaCO3(s) → CaO(s) + CO2(g)
b. C(s) + O2(g) → CO2(g)
c. CO2(g) + H2O(l) → H2CO3(aq)
d. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
77
If the equilibrium constant for the reaction of 2A → 2B is KC, what is the value for the equilibrium constant for the reaction of B → A?
(Note: For all equilibrium problems, the single direction arrow should be a double arrow representing an equilibrium.)
a. -2KC
b. 1/KC
c. (KC)1/2
d. 1/2KC
e. 1/(KC)1/2
f. (KC)2
g. 1/(KC)2
h. 2KC
78
If the value of KC for the reaction:
2O3(g) → 3O2(g) is 0.004289,
what is the value KP at a temperature of 48.14oC?
(Note: For all equilibrium problems, the single direction arrow should be a double arrow representing an equilibrium.)
79
If Qc is less than Kc, then the reaction will
a. shift to the right by increasing the concentration of the products.
b. shift to the right by increasing the concentration of the reactants
c. shift to the left by increasing the concentration of the products.
d. shift to the left by increasing the concentration of the reactants.
80
The value of Kc for the reaction of dinitrogen tetroxide to make nitrogen dioxide is 1.3617. The concentration of nitrogen dioxide 1.2949 M with no dinitrogen tetroxide. What is the equilibrium concentration (in M) of nitrogen dioxide?
81
The value of Kc for the reaction of phosphorus pentachloride to make phosphorus trichloride and chlorine is 2.2715. The concentration of phosphorus pentachloride 1.22592 M with no products. What is the equilibrium concentration (in M) of chlorine?
82
What is the value of KP for the reaction of nitrogen and oxygen to make dinitrogen monoxide if the equilibrium partial pressures of nitrogen is 1.2265 atm, the partial pressure of oxygen is 1.0906 atm and the partial pressure of dinitrogen monoxide is 0.0277 atm?
83
For the reaction of 2N2(g) + O2(g) → 2NO2(g), decreasing the temperature will cause the reaction to
(Note: For all equilibrium problems, the single direction arrow should be a double arrow representing an equilibrium.)
a. shift to the right by increasing the concentration of the products.
b. shift to the right by increasing the concentration of the reactants
c. shift to the left by increasing the concentration of the products.
d. shift to the left by increasing the concentration of the reactants.
e. not change as the change in temperature will not affect the equilibrium.
84
For the reaction of CO2(g) + NO(g) → NO2(g) + CO(g), if the pressure of the reaction vessel is increased by adding He(g), the equilibrium will be reestablished by the reaction
(Note: For all equilibrium problems, the single direction arrow should be a double arrow representing an equilibrium.)
a. shifting to the right by increasing the concentration of the products.
b. shifting to the right by increasing the concentration of the reactants
c. shifting to the left by increasing the concentration of the products.
d. shifting to the left by increasing the concentration of the reactants.
e. not changing as the change in pressure will not affect the equilibrium.
85
Which set is not a conjugate acid/base pair?
a. CH3COOH / CH3COO-
b. HCN / CN-
c. H2O / OH-
d. H2SO4 / HSO3-
86
What is the pH of a 1x10-5 M aqueous solution of nitric acid?
a. pH < 7
b. pH = 7
c. pH > 7
d. Cannot be determined
87
What is the percent ionization of a 0.356 M aqueous solution of acetic acid? Ka (CH3COOH) = 1.8x10-5
88
What is the pH of a 0.358 M aqueous solution of benzoic acid? Ka (C6H5COOH) = 6.5x10-5
89
What is the pH of a 0.377 M aqueous solution of oxalic acid? Ka1 = 6.5x10-2; Ka2 = 6.1x10-5
90
Which reaction corresponds to Ka2 for carbonic acid?
a. H2CO3(aq) → HCO3-(aq) + H+(aq)
b. H2CO3(aq) → CO32-(aq) + 2H+(aq)
c. HCO3-(aq) → CO32-(aq) + H+(aq)
d. CO32-(aq) + 2H+(aq) → H2CO3(aq)
91
What is the pH of a 0.361 M aqueous solution of NaCN? Ka (HCN) = 4.9x10-10
92
Aqueous ammonium nitrite will have a pH _____ 7. Enter either <, =, or >.
93
What is the pH of an aqueous solution made by combining 36.47 mL of a 0.3818 M ammonium chloride with 47.76 mL of a 0.3886 M solution of ammonia to which 4.299 mL of a 0.0764 M solution of NaOH was added?
94
What is the pH of an aqueous solution made by combining 44.96 mL of a 0.4429 M sodium formate with 40.11 mL of a 0.3291 M solution of formic acid?
95
What is the pH of an aqueous solution made by combining 13.19 mL of a 0.1939 M hydrochloric acid with 35.35 mL of a 0.3509 M solution of ammonia?
96
In a titration of 44.43 mL of 0.3896 M ammonia with 0.3896 M aqueous nitric acid, what is the pH of the solution when 44.43 mL of the acid have been added?
97
In a titration of 37.86 mL of 0.3855 M nitrous acid with 0.3855 M aqueous sodium hydroxide, what is the pH of the solution when 37.86 mL of the base have been added?
98
What is the pKa of HNO2? _____ Ka = 4.5x10-4. Use three digits for your answer.
99
Which base has the lowest pKa?
a. CH3NH2
b. C2H5NH2
c. C6H5NH2
d. NH3
100
In order to selectively precipitate barium ions from calcuim ions, what could you add?
a. either sodium carbonate or sodium fluoride
b. sodium fluoride but not sodium carbonate
c. sodium carbonate but not sodium fluoride
d. neither sodium carbonate nor sodium fluoride
101
What is the concentration of the calcium ion in a saturated solution of calcium fluoride that also contains 0.0100 M sodium fluoride
a. [Ca2+] greater than [F-]
b. [Ca2+] equal to [F-]
c. [Ca2+] less than [F-]
d. Cannot be determined without volumes
102
What is the molar solubility of silver sulfide? _____ Enter your answer with 3 significant digits with no units and the format of "1.00x10(-4)" for 1.00x10-4.
103
What kind of a solution do you have when you mix 10.0 mL of a 1x10-4 M silver nitrate with 10.0 mL of a 1x10-8 M sodium chloride?
a. There is no precipitate and the solution is saturated.
b. There is no precipitate and the solution is unsaturated.
c. There is a precipitate and the solution is saturated.
d. There is a precipitate and the solution is unsaturated.
104
Using Appendix 1 in your textbook, what is the standard change in entropy (in J/K) at 25oC of the reaction:
2CO(g) + O2(g) → 2CO2(g)?
105
What is the sign on the change in entropy for the process: 2N2(g) + O2(g)→ 2N2O(g)
a. entropy is increasing
b. entropy is unchanged
c. entropy is decreasing
d. entropy cannot be approximated
106
What is the order of the lowest entropy (1 = lowest) to highest entropy (3 = highest)?
Br2(g) 1 = lowest 3 = highest 2 = moderate
Cl2(g) 1 = lowest 3 = highest 2 = moderate
F2(g) 1 = lowest 3 = highest 2 = moderate
107
Which describes an endothermic system in which the entropy of the universe is increasing (spontaneous)?
a. Enthalpy of the surroundings decreases and the entropy of the system decreases
b. Enthalpy of the surroundings decreases and the entropy of the system increases
c. Enthalpy of the surroundings increases and the entropy of the system decreases
d. Enthalpy of the surroundings increases and the entropy of the system increases
108
Using Appendix 2 in your textbook, at what temperature (in K) will the reaction, 2H2O(l) → 2H2(g) + O2(g), change in spontaneity?
Assume standard change in enthalpy and standard change in entropy do not change with temperature.
109
Using Appendix 2 in your textbook, what is the value for the standard change in Gibbs free energy (in kJ) at 25oC of the reaction:
2NO(g) + N2(g) → 2N2O(g)?
110
Which combination will result in a system that is spontaneous at high temperatures only?
a. ΔHsys< 0 and ΔSsys< 0
b. ΔHsys< 0 and ΔSsys> 0
c. ΔHsys> 0 and ΔSsys< 0
d. ΔHsys> 0 and ΔSsys> 0
111
Given the Ka of benzoic acid from Chapter 16 in your textbook, what is the value of change in Gibbs free energy (in kJ/mol) at 25oC for this process?
112
How many electrons are transferred in the redox reaction taking place in acidic solution:
Sn2+(aq) + Cr2O72-(aq) → Cr3+(aq) + Sn4+(aq)?
113
What is the stoichiometric coefficient for the hydroxide ion in the balanced redox reaction of:
In+(aq) + ClO-(aq) → Cl-(aq) + In3+(aq) when balanced in basic solution?