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CHEM161 FINAL EXAM (PRACTICE)
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1. A 19.0-g sample of lithium is completely burned in air to form lithium oxide. The mass of lithium
oxide must be
A) less than 19.0 g.
B) greater than 19.0 g.
C) equal to 19.0 g.
D) all of the above.
E) none of the above.
____
2. A sample that cannot be separated into two or more substances by physical means is
A) a heterogeneous mixture.
B) a compound.
C) either a compound or an element.
D) an element.
E) a homogeneous mixture.
____
3. Which of the following is an example of a chemical change?
A) silver tarnishing
B) iodine sublimating
C) alcohol boiling
D) sucrose dissolving
E) sodium chloride melting
____
4. Two students determined the volume of a glass container three separate times (see table below).
The true volume of the container is 24.20 mL. Which statement correctly describes the students’
results?
Student A
24.3 mL
24.4 mL
24.5 mL
Student B
24.89 mL
24.87 mL
24.88 mL
A) Student A’s results are the most accurate. Student B’s results are the most
precise.
B) Student A’s results are the most accurate and precise.
C) Student B’s results are the most accurate and precise.
D) Student A’s results are the most precise. Student B’s results are the most
accurate.
E) The precision and accuracy of the two data sets are identical.
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5. Express the result of the following calculation in scientific notation: 0.0263 cm2 ÷ 88.2 cm
A)
B)
C)
D)
E)
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6. What is the best answer to the following expression involving a sum of measurements?
(85.430 cm + 0.400 cm + 31.3 cm)
A)
B)
C)
D)
E)
117 cm
117.1300 cm
117.13 cm
117.130 cm
117.1 cm
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7. The melting point of nitrogen is 63 K. What is this temperature in degrees Celsius?
A) 63°C
B) –336°C
C) –63°C
D) –210.°C
E) 483°C
____
8. A particular sheet of paper measures
paper in cm2? (2.54 cm = 1 in exactly)
A) 1.1  102 cm2
B) 4.4  101 cm2
C) 2.8  102 cm2
D) 1.7  101 cm2
E) 6.8 cm2
____
9. A 4.06 cm3 sample of solid sodium metal has a density of 0.968 g/cm3. What volume does this
sample of sodium occupy in its liquid state? The density of liquid sodium is 0.927 g/cm3.
A) 4.24 cm3
B) 3.89 cm3
C) 4.52 cm3
D) 3.64 cm3
E) 0.257 cm3
____
inches. What is the surface area of one side of the
10. The average speed of oxygen molecules at 690°C is 1.60  105 cm/s. Which of the following
calculations would convert this speed to units of miles per hour?
A)
B)
C)
D)
E)
____
11. Which one of the following lists gives the correct symbols for the elements phosphorus, potassium,
silver, chlorine, and sulfur?
A) P, Po, Ag, Cl, S
B) K, Ag, Po, Cl, S
C) P, K, Ag, Cl, S
D) Ph, K, Ag, S, Cl
E) Ph, Po, Ag, Cl, S
____
12. Which of the following conclusions regarding Rutherford’s gold foil experiment is not consistent
with the observations?
A) The nucleus occupies only a small portion of the space of an atom.
B) Most alpha particles travel straight through the gold foil.
C) The nucleus occupies a large amount of the atom space.
D) The nucleus, like the alpha particles used to bombard the gold foil, is positively
charged.
E) Wide angle deflections result from a collision of an alpha particle and a gold atom
nucleus.
____
13. Which nuclide has the same number of protons as
A)
?
B)
C)
D)
E)
____
14. Which of the following statements about different elements is incorrect?
A) Potassium is an alkali metal.
B) Fluorine is a halogen.
C) Aluminum is a transition element.
D) Barium is an alkaline earth metal.
E) Helium is a noble gas.
____
15. What is the formula of magnesium nitrite?
A) Mg(NO2)2
B) Mg3N2
C) Mg2(NO2)2
D) Mg2N3
E) Mg(NO2)3
____
16. Which is a correct balanced chemical equation corresponding to the following description of a
chemical reaction?
Hydrochloric acid reacts with magnesium metal to produce aqueous magnesium chloride and
hydrogen gas.
A) 2HCl(aq) + Mg(s)  MgCl2(aq) + 2H(g)
B) 2HCl(aq) + Mg(s)  MgCl2(aq) + H2(g)
C) 2HCl(aq) + Mg(s)  MgCl(aq) + H2(g)
D) 2HCl(aq) + Mg(aq)  MgCl2(s) + H2(g)
E) HCl(aq) + Mg(s)  MgCl(aq) + H(g)
____
17. Which of the following chemical equations is not balanced?
A) NH4NO3  N2O + 2H2O
B) C12H22O11  12C + 11H2O
C) 2NH4SCN + Ba(OH)2 • 8H2O  2NH3 + 10H2O + Ba(SCN)2
D) (NH4)2Cr2O7  N2O + Cr2O3 + 4H2O
E) 2Mg + CO2  2MgO + C
____
18. The formula mass of zinc acetate trihydrate, Zn(CH3COO)2 • 3H2O, is
A) 321 amu.
B) 184 amu.
C) 268 amu.
D) 238 amu.
E) 114 amu.
____
19. How many molecules are there in 192 g of citric acid, C6H8O7?
A) (6.02  1023) / 192
B) 192
C) 6.02  1023
D) 96.0
E) 192  (6.02  1023)
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20. What is the percent by mass oxygen in (NH4)2SO3?
A) 41.3 %
B) 20.7 %
C) 54.0 %
D) 42.0 %
E) 1.00 %
____
21. A compound composed of only C and F contains 17.39 % C by mass. What is its empirical
formula?
A) CF3
B) CF
C) C2F
D) CF4
E) CF2
____
22. The empirical formula of styrene is CH. An experimental determination of the molar mass of
styrene by a student yields the value of 104 g/mol. What is the molecular formula of styrene?
A) C5H10
B) CH
C) C8H8
D) C3H8
E) C6H9
____
23. Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows:
Cu2S(s) + O2(g)  2Cu(s) + SO2(g)
If 0.680 kg of copper(I) sulfide reacts with excess oxygen, what mass of copper metal may be
produced?
A) 0.680 kg
B) 0.136 kg
C) 0.271 kg
D) 0.543 kg
E) 1.36 kg
____
24. Which of the following solutions would be expected to be the best conductor of an electric current
at room temperature?
A) 0.10 M Na2SO4
B) 1.0 M CH3COOH
C) 0.10 M NaCl
D) 0.10 M CO(NH2)2
E) 0.10 M CH3COOH
____
25. Identify the spectator ion(s) in the following reaction.
Cu(OH)2(s) + 2H+(aq) + 2Cl–(aq)  Cu2+(aq) + 2Cl–(aq) + 2H2O(l)
A)
B)
C)
D)
E)
Cu2+ and Cl–
Cu2+
Cu(OH)2
Cl–
H+ and Cl–
____
26. Which of the following is a weak electrolyte in aqueous solution?
A) Mg(OH)2
B) NH3
C) LiOH
D) RbOH
E) Sr(OH)2
____
27. All the following are oxidation–reduction reactions except
A) H2(g) + F2(g)  2HF(g).
B) Ca(s) + H2(g)  CaH2(s).
C) 2K(s) + 2H2O(l)  2KOH(aq) + H2(g).
D) 6Li(s) + N2(g)  2Li3N(s).
E) Mg3N2(s) + 6H2O(l)  3Mg(OH)2(s) + 2NH3(g).
____
28. What is the oxidation number of each O in BaFeO4?
A) +6
B) +2
C) -2
D) +3
E) 0
____
29. A 29.0-g sample of NaOH is dissolved in water, and the solution is diluted to give a final volume
of 1.60 L. The molarity of the final solution is
A) 18.1 M.
B) 0.453 M.
C) 0.725 M.
D) 0.0552 M.
E) 0.862 M.
____
30. What mass of oxalic acid dihydrate, H2C2O4 · 2H2O, is required to prepare 250.0 mL of a 1.32 M
solution of oxalic acid?
A) 126 g
B) 41.6 g
C) 119 g
D) 166 g
E) 29.7 g
____
31. What is the final concentration of HCl in a solution prepared by addition of 930.0 mL of 8.77 M
HCl to 468.0 mL of 3.22 M HCl? Assume volumes are additive.
A) 6.00 M
B) 0.00858 M
C) 12.0 M
D) 6.91 M
E) 5.08 M
____
32. In a volumetric analysis experiment, an acidic aqueous solution of methanol (CH3OH) is titrated
with a solution of potassium dichromate (K2Cr2O7) according to the following balanced chemical
equation:
2K2Cr2O7(aq) + 8H2SO4(aq) + 3CH3OH(aq)  2Cr2(SO4)3(aq) + 11H2O(l) + 3HCOOH(aq) +
2K2SO4(aq)
It required 43.91 mL of 0.0435 M K2Cr2O7 to reach the endpoint. What mass of CH3OH was
present initially?
A) 0.0918 g
B) 2.09 g
C) 0.929 g
D) 0.0612 g
E) 0.0408 g
____
33. A flexible vessel contains 32.00 L of gas at a pressure of 1.59 atm. Under conditions of constant
temperature and moles of gas, what is the volume of the gas when the pressure of the vessel is
decreased by a factor of three?
A) 96.1 L
B) 10.7 L
C) 0.0104 L
D) 32 L
E) 4.80 L
____
34. How many moles of gas are in a gas sample occupying 0.738 L at 135 mmHg and 30°C?
A)
B)
C)
D)
E)
190 mol
4.01 mol
40.5 mol
0.00527 mol
0.000433 mol
____
35. The density of a gas is 1.96 g/L at STP. What is its molar mass?
A) 65.2 g/mol
B) 58.9 g/mol
C) 11.4 g/mol
D) 22.4 g/mol
E) 43.9 g/mol
____
36. What is the total volume of gases produced at 819 K and 1.00 atm pressure when 320 g of
ammonium nitrite undergoes the following decomposition reaction?
NH4NO2(s)  N2(g) + 2H2O(g)
A)
B)
C)
D)
E)
3  22.4 L
22.4 L
15  22.4 L
5  22.4 L
45  22.4 L
____
37. Which of the following is included as a postulate in the kinetic molecular theory of an ideal gas?
A) Collisions between molecules are all elastic.
B) All molecules move randomly in zigzag directions.
C) The distance between gas molecules is small compared with the size of the
molecule.
D) All the molecules have the same velocity.
E) In an average collision between molecules, both molecules have the same kinetic
energy.
____
38. Which of the following gases will have the slowest rate of effusion at constant temperature?
A) H2
B) F2
C) Ne
D) SO3
E) CF4
____
39. Real gases deviate from ideal behavior for two reasons: (1) real gas molecules have intermolecular
forces, and (2) real gas molecules have
A) pressures within the chemical bonds.
B) nonzero molecular volumes.
C) ionization energies.
D) molecular vibrations.
E) a distribution of molecular speeds.
____
40. Given the thermochemical equation
2Al(s) + O2(g)  Al2O3(s); H = –1676 kJ
find H for the following reaction.
2Al2O3(s)  4Al(s) + 3O2(g)
A)
B)
C)
D)
E)
____
838 kJ
1676 kJ
–1676 kJ
3352 kJ
–838 kJ
41. What mass of hydrogen is consumed when 587.9 kJ of energy is evolved from the combustion of a
mixture of H2(g) and O2(g)?
H2(g) + O2(g)  H2O(l); H° = –285.8 kJ
A)
B)
C)
D)
E)
4.147 g
2.073 g
0.2412 g
6.162 g
2.131 g
____
42. The quantity of heat required to raise the temperature of a sample of a substance by 1°C is the
sample’s
A) work.
B) calorimetry.
C) heat capacity.
D) specific heat.
E) enthalpy.
____
43. A 100 g sample of each of the following metals is heated from 35C to 45C. Which metal
absorbs the lowest amount of heat energy?
Metal
copper
magnesium
mercury
silver
lead
A)
B)
C)
D)
E)
____
Specific Heat
0.385 J/(g°C)
1.02 J/(g°C)
0.138 J/(g°C)
0.237 J/(g°C)
0.129 J/(g°C)
lead
magnesium
silver
mercury
copper
44. Exactly 105.2 J will raise the temperature of 10.0 g of a metal from 25.0°C to 60.0°C. What is the
specific heat capacity of the metal?
A) 0.301 J/(g°C)
B)
C)
D)
E)
____
3.33 J/(g°C)
29.3 J/(g°C)
25.2 J/(g°C)
none of these
45. Given:
Pb(s) + PbO2(s) + 2H2SO4(l)  2PbSO4(s) + 2H2O(l); H° = –509.2 kJ
SO3(g) + H2O(l)  H2SO4(l); H° = –130. kJ
determine H° for the following thermochemical equation.
Pb(s) + PbO2(s) + 2SO3(g)  2PbSO4(s)
A)
B)
C)
D)
E)
3.77 103 kJ
–521 kJ
–3.77  103 kJ
–639 kJ
–769 kJ
____
46. Which of the following species does not have a standard enthalpy of formation equal to zero at
25°C?
A) Cl2(l)
B) N2(g)
C) Fe(s)
D) H+(aq)
E) S8(s)
____
47. What is the frequency of a photon having a wavelength of 954.9 nm? (
)
A) 3.14  10–4 Hz
B) 1.44  1027 Hz
C) 3.14  1014 Hz
D) 2.08  10–37 Hz
E) 2.08  10–19 Hz
____
48. When an electron in an atom makes a transition from n = 6 to n = 4, which of the following
statements is/are correct?
I.
II.
III.
IV.
V.
Energy is emitted.
Energy is absorbed.
The electron loses energy.
The electron gains energy.
The electron cannot make this transition.
A) I and III
B) I and IV
C) II and IV
,
D) II and III
E) III
____
49. What is the frequency of light emitted when the electron in a hydrogen atom undergoes a transition
from level
(
)
A)
B)
C)
D)
E)
____
50. Which of the following combinations of quantum numbers is permissible?
A) n = 1, l = 2, ml = 0, ms =
B) n = 3, l = 2, ml = 1, ms =
C) n = 3, l = 3, ml = 1, ms =
D) n = 2, l = 1, ml = –1, ms = 0
E) n = 4, l = 3, ml = 4, ms =
CHEM161 FINAL EXAM (PRACTICE)
Answer Section
1. ANS: B
PTS: 1
DIF: easy
REF: 1.3
OBJ: Apply the law of the conservation of mass. (Example 1.1)
TOP: general concepts | matter
2. ANS: C
PTS: 1
DIF: easy
REF: 1.4
OBJ: Describe the classifications of matter: elements, compounds, and mixtures (heterogeneous
and homogeneous). TOP: general concepts | matter
KEY: states of matter
MSC: general chemistry
3. ANS: A
PTS: 1
DIF: easy
REF: 1.4
OBJ: Understand the difference between chemical changes (chemical reactions) and physical
changes.
TOP: general concepts | matter
KEY: physical and chemical change
MSC: general chemistry
4. ANS: A
PTS: 1
DIF: easy
REF: 1.5
OBJ: Define and use the terms precision and accuracy when describing measured quantities.
TOP: general concepts | measurement
5. ANS: D
PTS: 1
DIF: easy
REF: 1.5
OBJ: Know how to represent numbers using scientific notation.
TOP: general concepts | measurement
KEY: significant figures | scientific notation
MSC: general chemistry
6. ANS: E
PTS: 1
DIF: easy
REF: 1.5
OBJ: Use significant figures in calculations. (Example 1.2)
TOP: general concepts | measurement
KEY: significant figures
MSC: general chemistry
7. ANS: D
PTS: 1
DIF: easy
REF: 1.6
OBJ: Convert from one temperature scale to another. (Example 1.3)
TOP: general concepts | measurement
KEY: SI unit | temperature
MSC: general chemistry
8. ANS: C
PTS: 1
DIF: difficult
REF: 1.7
OBJ: Define and provide examples of derived units.
TOP: general concepts | measurement
MSC: general chemistry
9. ANS: A
PTS: 1
DIF: difficult
REF: 1.8
OBJ: Use density to relate mass and volume.
TOP: general concepts | measurement
10. ANS: C
PTS: 1
DIF: moderate
REF: 1.8
OBJ: Apply dimensional analysis to solving numerical problems.
TOP: general concepts | measurement
KEY: factor label method
MSC: general chemistry
11. ANS: C
PTS: 1
DIF: easy
REF: 2.1
OBJ: Recognize the atomic symbols of the elements.
TOP: early atomic theory | atomic theory of matter
KEY: atomic symbol
MSC: general chemistry
12. ANS: C
PTS: 1
DIF: easy
REF: 2.2
OBJ: Describe Rutherford's experiment that led to the nuclear model of the atom.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
TOP: early atomic theory | atomic theory of matter
ANS: E
PTS: 1
DIF: easy
REF: 2.3
OBJ: Write the nuclide symbol for a given nuclide.
TOP: early atomic theory | atomic theory of matter
KEY: nuclear structure
MSC: general chemistry
ANS: C
PTS: 1
DIF: easy
REF: 2.5
OBJ: Find the main-group and transition elements on the periodic table.
TOP: early atomic theory | periodic table MSC: general chemistry
ANS: A
PTS: 1
DIF: easy
REF: 2.8
OBJ: Write the formula of an ionic compound from its name. (Example 2.5)
TOP: early atomic theory | chemical substance
KEY: nomenclature of simple compound | ionic compound
MSC: general chemistry
ANS: B
PTS: 1
DIF: moderate
REF: 2.9
OBJ: Write chemical equations using appropriate phase labels,symbols of reactions conditions,
and the presence of a catalyst.
TOP: early atomic theory | chemical equation
KEY: balancing chemical equation
MSC: general chemistry
ANS: D
PTS: 1
DIF: easy
REF: 2.10
OBJ: Determine if a chemical reaction is balanced.
TOP: early atomic theory | chemical equation
KEY: balancing chemical equation
MSC: general chemistry
ANS: D
PTS: 1
DIF: easy
REF: 3.1
OBJ: Calculate the formula mass from a formula. (Example 3.1)
TOP: stoichiometry | mass and moles of substance
KEY: formula mass
MSC: general chemistry
ANS: C
PTS: 1
DIF: easy
REF: 3.2
OBJ: Calculate the number of molecules in a given mass of substance. (Example 3.6)
TOP: stoichiometry | mass and moles of substance
KEY: mole | mole calculations
MSC: general chemistry
ANS: A
PTS: 1
DIF: easy
REF: 3.3
OBJ: Calculate the percentage composition of the elements in a compound. (Example 3.7)
TOP: stoichiometry | determining chemical formulas
ANS: A
PTS: 1
DIF: easy
REF: 3.5
OBJ: Determine the empirical formula from the percentage composition. (Example 3.11)
TOP: stoichiometry | determining chemical formulas
KEY: empirical formula
MSC: general chemistry
ANS: C
PTS: 1
DIF: easy
REF: 3.5
OBJ: Understand the relationship between the molecular mass of a substance and its empirical
formula mass.
TOP: stoichiometry | determining chemical formulas
KEY: molecular formula
MSC: general chemistry
ANS: D
PTS: 1
DIF: easy
REF: 3.7
OBJ: Relate the quantities of two reactants or two products. (Example 3.14)
TOP: stoichiometry | stoichiometry calculation
KEY: amounts of substances
MSC: general chemistry
ANS: A
PTS: 1
DIF: easy
REF: 4.1
OBJ: Compare the properties of solutions that contain strong electrolytes and weak electrolytes.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
TOP:
MSC:
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OBJ:
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KEY:
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MSC:
ANS:
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MSC:
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MSC:
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TOP:
MSC:
ANS:
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ANS:
OBJ:
KEY:
ANS:
OBJ:
KEY:
ANS:
OBJ:
TOP:
MSC:
chemical reactions | ions in aqueous solution
KEY: electrolyte
general chemistry
D
PTS: 1
DIF: easy
REF: 4.2
From the complete ionic equation, write the net ionic equation.
chemical reactions | ions in aqueous solution
ionic equation | net ionic equation MSC: general chemistry
B
PTS: 1
DIF: easy
REF: 4.4
Distinguish between a strong base and a weak base and the solutions they form.
chemical reactions | types of chemical reactions
acid-base reaction | weak base
MSC: general chemistry
E
PTS: 1
DIF: easy
REF: 4.5
Define an oxidation-reduction reaction.
chemical reactions | types of chemical reactions
oxidation-reduction reaction
MSC: general chemistry
C
PTS: 1
DIF: moderate
REF: 4.5
Learn the oxidation-number rules.
chemical reactions | types of chemical reactions
B
PTS: 1
DIF: easy
REF: 4.7
Calculate the molarity from mass and volume. (Example 4.9)
chemical reactions | working with solutions
KEY: concentration
general chemistry
B
PTS: 1
DIF: moderate
REF: 4.7
Use molarity as a conversion factor. (Example 4.10)
chemical reactions | working with solutions
KEY: concentration
general chemistry
D
PTS: 1
DIF: difficult
REF: 4.8
Perform calculations associated with dilution.
chemical reactions | working with solutions
KEY: diluting solutions
general chemistry
A
PTS: 1
DIF: moderate
REF: 4.10
Calculate the quantity of substance in a titrated solution. (Example 4.14)
chemical reactions | quantitative analysis
KEY: volumetric analysis
general chemistry
A
PTS: 1
DIF: easy
REF: 5.2
Use Boyle's law. (Example 5.2)
TOP: phases | gas
D
PTS: 1
DIF: easy
REF: 5.3
Use the ideal gas law. (Example 5.6)
TOP: phases | gas
ideal gas law | calculations with the ideal gas law
MSC: general chemistry
E
PTS: 1
DIF: easy
REF: 5.3
Determine the molecular mass of a vapor. (Example 5.8) TOP: phases | gas
ideal gas law | gas density
MSC: general chemistry
E
PTS: 1
DIF: moderate
REF: 5.4
Solving stoichiometry problems involving gas volumes. (Example 5.9)
phases | gas KEY: ideal gas law | stoichiometry and gas volumes
general chemistry
37. ANS: A
PTS: 1
DIF: easy
REF: 5.6
OBJ: List the five postulates of the kinetic theory.
TOP: phases | gas
KEY: kinetic theory of an ideal gas | postulates of kinetic theory
MSC: general chemistry
38. ANS: E
PTS: 1
DIF: easy
REF: 5.7
OBJ: Calculate the ratio of effusion rates of gases. (Example 5.13)
TOP: phases | gas KEY: molecular speed | effusion
MSC: general chemistry
39. ANS: B
PTS: 1
DIF: easy
REF: 5.8
OBJ: Explain how and why a real gas is different from an ideal gas.
TOP: phases | gas KEY: real gases
MSC: general chemistry
40. ANS: D
PTS: 1
DIF: easy
REF: 6.4
OBJ: Manipulate a thermochemical equation using these rules. (Example 6.3)
TOP: thermochemistry | heats of reaction KEY: thermochemical equation | enthalpy of reaction
MSC: general chemistry
41. ANS: A
PTS: 1
DIF: easy
REF: 6.5
OBJ: Calculate the heat absorbed or evolved from a reaction given its enthalpy of reaction and
the mass of a reactant or product. (Example 6.4)
TOP: thermochemistry | heats of reaction
42. ANS: C
PTS: 1
DIF: easy
REF: 6.6
OBJ: Define heat capacity and specific heat.
TOP: thermochemistry | heats of reaction KEY: calorimetry | heat capacity
MSC: general chemistry
43. ANS: A
PTS: 1
DIF: easy
REF: 6.6
OBJ: Relate the heat absorbed or evolved to the specific heat, mass, and temperature change.
TOP: thermochemistry | heats of reaction
44. ANS: A
PTS: 1
DIF: easy
REF: 6.6
OBJ: Calculate using this relation between heat and specific heat. (Example 6. 5)
TOP: thermochemistry | heats of reaction KEY: calorimetry | specific heat
MSC: general chemistry
45. ANS: E
PTS: 1
DIF: moderate
REF: 6.7
OBJ: Apply Hess's law to obtain the enthalpy change for one reaction from the enthalpy changes
of a number of other reactions. (Example 6.7)
TOP: thermochemistry | heats of reaction KEY: Hess's law
MSC: general chemistry
46. ANS: A
PTS: 1
DIF: easy
REF: 6.8
OBJ: Define standard state and reference form.
TOP: thermochemistry | heats of reaction KEY: standard enthalpies of formation
MSC: general chemistry
47. ANS: C
PTS: 1
DIF: easy
REF: 7.1
OBJ: Relate the wavelength, frequency, and speed of light. (Examples 7.1 and 7.2)
TOP: atomic theory | light
KEY: electromagnetic radiation
MSC: general chemistry
48. ANS: A
PTS: 1
DIF: easy
REF: 7.3
OBJ: Relate the energy of a photon to the associated energy levels of an atom.
TOP: atomic theory | light
49. ANS: E
PTS: 1
DIF: moderate
REF: 7.3
OBJ:
TOP:
MSC:
50. ANS:
OBJ:
TOP:
MSC:
Determine the wavelength or frequency of a hydrogen atom transition. (Example 7.4)
atomic theory | light
KEY: Bohr theory | atomic line spectra
general chemistry
B
PTS: 1
DIF: easy
REF: 7.5
Apply the rules for quantum numbers. (Example 7.6)
atomic theory | quantum mechanics
KEY: quantum numbers
general chemistry