General Chemistry I Final Test Solutions - 3150 Verified Questions

General Chemistry I Final Test Solutions

Course Introduction

General Chemistry I is an introductory course that covers the fundamental principles of chemistry, including atomic and molecular structure, periodic properties of the elements, chemical bonding, stoichiometry, states of matter, thermochemistry, and basic chemical reactions. Students will develop problem-solving skills and gain hands-on laboratory experience to better understand chemical concepts and their real-world applications. This course lays the groundwork for further study in chemistry and related scientific disciplines.

Recommended Textbook Chemistry 12th Edition by Raymond Chang

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25 Chapters

3150 Verified Questions

3150 Flashcards

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Chapter 1: Chemistry: The Study of Change

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Sample Questions

Q1) What is the density of a salt solution if 75.0 mL of the solution has a mass of 32.0 g

A) 0.127 g/mL

B) 0.227 g/mL

C) 0.327 g/mL

D) 0.427 g/mL

E) None of the above

Answer: D

Q2) Convert 4.89 mm to µm.

A) 4.89 x 10^-6 µm

B) 4.89 x 10^-3 µm

C) 4.89 x 10³ µm

D) 4.89 x 10⁶ µm

E) 4.89 x 10⁹ µm

Answer: C

Q3) Brewed coffee is a pure substance.

A)True

B)False

Answer: False

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Chapter 2: Atoms Molecules and Ions

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Sample Questions

Q1) Of the following which is the formula of an anion that contains a metal

A) Cr₂O₇^2-

B) NH₄⁺

C) SO₄^2-

D) SO₃^2-

E) NO₃^-

Answer: A

Q2) Use the periodic table above to identify where the alkali metals are located.

A) Group 1A

B) Group 2B

C) Group 3A

D) Group 7A

E) Group 8A

Answer: A

Q3) An ion is an atom or group of atoms that has a net positive or negative charge.

A)True

B)False

Answer: True

Q4) What are the two different ions present in the compound FeCl₃

Answer: \(Fe^{2+}, Cl^-\)

Page 4

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) What is the coefficient of H₂O when the equation below is properly balanced ___ PCl₃(l) + ___ H₂O(l) \(\rarr\) ___ H₃PO₃(aq) + ___ HCl(aq)

A) 1

B) 2

C) 3

D) 5

E) none of these

Answer: C

Q2) A compound with an empirical formula of C₂H₂Br₃ has a molar mass of 531.47 g/mol. What is the molecular formula

A) C₂H₂Br₃

B) C₄H₄Br₆

C) CHBr

D) C₄H₄Br₃

E) C₆H₆Br₉

Answer: B

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Page 5

Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) How many total electrons are transferred in the following reaction

2Na(s) + Cl₂(g) \(\rarr\) 2NaCl(s)

A) 1

B) 2

C) 3

D) 4

E) 5

Q2) What mass of K₂CO₃ is needed to prepare 200. mL of a solution having a potassium ion concentration of 0.150 M

A) 4.15 g

B) 10.4 g

C) 13.8 g

D) 2.07 g

E) 1.49 g

Q3) A solution is a homogeneous mixture of two or more substances.

A)True B)False

Q4) H₂CO₃ is an example of a diproticacid.

A)True B)False

6

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Chapter 5: Gases

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Sample Questions

Q1) The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25^\(\circ\)C is required for burning 1.00 L of hexane (C₆H₁₄, density = 0.660 g/mL) completely, yielding carbon dioxide and water

A) 187 L

B) 712 L

C) 894 L

D) 1780 L

E) 8490 L

Q2) A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at -4.0^\(\circ\)C. Which of these choices is its molecular formula

A) NO

B) NO₂

C) N₃O₆

D) N₂O₄

E) N₂O₅

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Page 7

Chapter 6: Thermochemistry

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Sample Questions

Q1) The specific heat of gold is 0.129 J/g·^\(\circ\)C. What is the molar heat capacity of gold

A) 0.039 J/mol·^\(\circ\)C

B) 0.129 J/mol·^\(\circ\)C

C) 25.4 J/mol·^\(\circ\)C

D) 39.0 kJ/mol·^\(\circ\)C

E) 197 J/mol·^\(\circ\)C

Q2) Which of the following processes always results in an increase in the energy of a system

A) The system loses heat and does work on the surroundings.

B) The system gains heat and does work on the surroundings.

C) The system loses heat and has work done on it by the surroundings.

D) The system gains heat and has work done on it by the surroundings.

E) None of these is always true.

Q3) The heat capacity of 10.0 g of water is 83.7 J/^\(\circ\)C.

A)True

B)False

Q4) The work done on the surroundings by the expansion of a gas is w = -PDV.

A)True

B)False

Page 8

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Chapter 7: Quantum Theory and the Electronic Structure of Atoms

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Sample Questions

Q1) "No two electrons in an atom can have the same four quantum numbers" is a statement of

A) the Pauli exclusion principle.

B) Bohr's equation.

C) Hund's rule.

D) de Broglie's relation.

E) Dalton's atomic theory.

Q2) An electron gains energy in the transition from a 6s subshell to a 5d subshell.

A)True

B)False

Q3) Which element has the following ground-state electron configuration

[Ar]4s²3d¹⁰4p⁵

A) arsenic

B) bromine

C) iodine

D) selenium

E) tellurium

Q4) An electron gains energy in the transition from a 4d subshell to a 5s subshell.

A)True B)False

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Chapter 8: Periodic Relationships Among the Elements

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Sample Questions

Q1) The law of octaves states that every eighth element has similar properties when arranged in order of increasing

A) nuclear binding energy.

B) number of electrons.

C) number of neutrons.

D) atomic mass.

E) atomic number.

Q2) Which two electron configurations represent elements that would have similar chemical properties

(1) 1s²2s²2p⁴ (2) 1s²2s²2p⁵ (3) [Ar]4s²3d⁵ (4) [Ar]4s²3d¹⁰4p⁵

A) (1) and (2)

B) (1) and (3)

C) (2) and (3)

D) (2) and (4)

E) (3) and (4)

Q3) Amphoteric oxides exhibit both acidic and basic properties.

A)True

B)False

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Chapter 9: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) Which one of the following is most likely to be a covalent compound

A) KF

B) CaCl₂

C) SF₄

D) Al₂O₃

E) CaSO₄

Q2) Which of the following solids would have the highest melting point

A) NaI

B) NaF

C) MgO

D) MgCl₂

E) KF

Q3) Which one of the following compounds utilizes both ionic and covalent bonding

A) C₁₀H₂₂O

B) NH₃

C) Na₂S

D) NH₄NO₃

E) K₃N

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Chapter 10: Chemical Bonding II: Molecular Geometry and Hybridization

of Atomic

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Sample Questions

Q1) The hybridization of the central nitrogen atom in the molecule N₂O is A)sp.

B) sp².

C) sp³.

D) sp³d.

E) sp³d².

Q2) Predict the geometry and polarity of the CS₂ molecule.

A) linear, polar

B) linear, nonpolar

C) tetrahedral, nonpolar

D) bent, nonpolar

E) bent, polar

Q3) Which of the following species have the same geometries

A) NH₂^- and H₂O

B) NH₂^- and BeH₂

C) H₂O and BeH₂

D) NH₂^-, H₂O, and BeH₂

Q4) A species with a bond order of 1/2 may be stable.

A)True

B)False

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Chapter 11: Intermolecular Forces and Liquids and Solids

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Sample Questions

Q1) At a given temperature CCl₄ has a weaker surface tension than H₂O.

A)True

B)False

Q2) Which two properties are more typical of molecular compounds than of ionic compounds

1. They are gases or liquids at room temperature.

2. They have high melting points.

3. Solids do not conduct electricity, but liquids do.

4. Atoms share electrons.

A) 1 and 4

B) 1 and 3

C) 2 and 3

D) 2 and 4

E) 3 and 4

Q3) H₂S has stronger intermolecular forces of attraction than H₂Se.

A)True

B)False

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Page 13

Chapter 12: Physical Properties of Solutions

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Sample Questions

Q1) What is the mass percent CH₃OH of a 0.256 m CH₃OH(aq) solution

A) 0.819 %

B) 0.992 %

C) 1.23 %

D) 1.29 %

E) 1.51 %

Q2) A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol) to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol).

Calculate the mole fraction and molality of benzene in this solution.

A) Mole fraction = 0.0769; molality = 0.789 m

B) Mole fraction = 0.0869; molality = 0.789 m

C) Mole fraction = 0.0769; molality = 0.989 m

D) Mole fraction = 0.0869; molality = 0.989 m

E) None of the above

Q3) The vapor pressure of a solution depends on the chemical nature of the solvent.

A)True

B)False

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Chapter 13: Chemical Kinetics

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Sample Questions

Q1) B is a catalyst in the following mechanism: \(\begin{array}{lr} \mathrm{A} \rightarrow \mathrm{C}+\mathrm{B} & \text { slow } \\ \mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}+\mathrm{E} & \text { fast } \end{array}\)

A)True

B)False

Q2) The reaction 2NO₂(g) \(\rarr\) 2NO(g) + O₂(g) is suspected to be second order in NO₂. Which of the following kinetic plots would be the most useful to confirm whether or not the reaction is second order

A) A plot of [NO₂]^-1 vs. t

B) A plot of ln [NO₂]^-1 vs. t

C) A plot of ln [NO₂] vs. t

D) A plot of [NO₂]² vs. t

E) A plot of [NO₂] vs. t

Q3) In the reaction, 2N₂O \(\rarr\) 2N₂ + O₂, oxygen and nitrogen gases are formed at the same rate (mol/L·s).

A)True

B)False

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Page 15

Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) The equilibrium constant expression for the reaction 2BrF₅ (g) \(\rightleftharpoons\) Br₂ (g) + 5F₂ (g) is

A) K_c = [Br₂] [F₂] / [BrF₅]

B) K_c = [Br₂] [F₂]⁵ / [BrF₅]²

C) K_c = [Br₂] [F₂]² / [BrF₅]⁵

D) K_c = [BrF₅]² / [Br₂][F₂]⁵

E) K_c = 2[BrF₅]² / ([Br₂] *5[F₂]⁵)

Q2) Concerning the following reaction at equilibrium: 3Fe(s) + 4H₂O(g) Fe₃O₄(s) + 4H₂(g), increasing the concentration of the Fe(s) would:

A) Shift the equilibrium to the right

B) Shift the equilibrium to the left

C) Increase the value of the equilibrium constant, K

D) Decrease the value of the equilibrium constant, K

E) Cause no change

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Chapter 15: Acids and Bases

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Sample Questions

Q1) Calculate the H⁺ ion concentration in a 8.8 * 10^-4 M Ca(OH)₂ solution.

A) 8.8 * 10^-4 M

B) 1.8 * 10^-3 M

C) 2.2 * 10^-11 M

D) 1.1 * 10^-11 M

E) 5.7 * 10^-12 M

Q2) If the pH of pure water is 7.0, the hydroxide ion concentration in pure water is 1 * 10^-7 M.

A)True

B)False

Q3) Which solution will have the lowest pH

A) 0.25 M HClO

B) 0.25 M HClO₂

C) 0.25 M HClO₃

D) 0.25 M HClO₄

E) 0.25 M NaClO₄

Q4) H₂SO₄ is a stronger acid than HSO₄^-.

A)True

B)False

17

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Chapter 16: Acid-Base Equilibria and Solubility Equilibria

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Sample Questions

Q1) The solubility product for barium sulfate is 1.1 * 10^-10. Calculate the molar solubility of barium sulfate.

A) 5.5 * 10^-11 mol/L

B) 1.1 * 10^-5 mol/L

C) 2.1 * 10^-5 mol/L

D) 1.1 * 10^-10 mol/L

E) 2.2 * 10^-10 mol/L

Q2) Within what pH range is a HOCl - NaOCl buffer effective

A) pH 2.0 - pH 4.0

B) pH 7.5 - pH 9.5

C) pH 6.5 - pH 8.5

D) pH 6.5 - pH 9.5

E) pH 1.0 - pH 14.0

Q3) For which type of titration will the pH be neutral at the equivalence point

A) Strong acid vs. strong base.

B) Strong acid vs. weak base.

C) Weak acid vs. strong base.

D) All of the above.

E) None of the above.

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Page 18

Chapter 17: Entropy Free Energy and Equilibrium

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Sample Questions

Q1) For the reaction 2NO(g) + O₂(g) \(\rarr\) 2NO₂(g) if initially P(NO) = 1.5 atm, P(O₂) = 1.4 atm, and P(NO₂) = 2.0 atm, calculate \(\Delta\)G for this reaction at 25^\(\circ\)C. The following data is valid at 25^\(\circ\)C: \(\begin{array}{|c|c|} \hline & \Delta \mathrm{G}_{\mathrm{f}}{ }^{\circ}(\mathrm{kJ} / \mathrm{mol}) \\

\hline \mathrm{NO} & 86.7 \\ \hline \mathrm{NO}_{2} & 51.8 \\ \hline \end{array}\)

A) -69.9 kJ/mol

B) -69.2 kJ/mol

C) 522.1 kJ/mol

D) -79.9 kJ/mol

E) -35.0 kJ/mol

Q2) The standard entropy of any pure substance is 0 J/mol. A)True B)False

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Page 19

Chapter 18: Electrochemistry

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Sample Questions

Q1) Consider the following reaction: 2Fe²⁺(aq) + Cu²⁺ \(\rarr\) 2Fe³⁺(aq) + Cu.When the reaction comes to equilibrium, what is the cell voltage

A) 0.43 V

B) 1.11 V

C) 0.78 V

D) -0.43 V

E) 0 V

Q2) How many coulombs (C) of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca²⁺ ion to calcium metal

A) 190,000 C

B) 85,000 C

C) 21,000 C

D) 42,500 C

E) 0.88 C

Q3) H₂(g) will form when Sn is placed in 1.0 M HCl.

A)True

B)False

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Chapter 19: Nuclear Chemistry

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Sample Questions

Q1) As a result of beta decay, the product nucleus is

A) one atomic number lower than the original element.

B) two atomic numbers higher than the original element.

C) one atomic number higher than the original element.

D) two atomic numbers lower than the original element.

E) four atomic numbers lower than the original element.

Q2) Which of the following nuclear processes results in an increase of atomic number in the product element formed

I. Alpha emission

II. Beta emission

III. Positron emission

IV. Electron capture

A) I and II

B) III and IV

C) I, II, and III

D) II only

E) IV only

Q3) Calcium-45 is more stable than calcium-44.

A)True

B)False

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Chapter 20: Chemistry in the Atmosphere

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Sample Questions

Q1) In order for a gas to be a "greenhouse gas" it must

A) transmit visible light and absorb infrared radiation.

B) be radioactive.

C) transmit infrared light and absorb visible light.

D) be combustible.

E) absorb both visible light and infrared radiation.

Q2) What mass of solid CaO is needed to remove the sulfur dioxide from 1.0 * 10⁶ m³ of air having an SO₂ concentration of 1.5 * 10^-9 M Assume that the reaction leading to removal of the sulfur dioxide is CaO(s) + SO₂(g) \(\rarr\) CaCO₃(s).

A) 56 g

B) 96 g

C) 37 g

D) 84 g

E) 43 g

Q3) The following balanced equation shows what happens to nitrogen dioxide in sunlight.NO₂(g) + hn \(\rarr\) NO(g) + O(g)

A)True

B)False

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Page 22

Chapter 21: Metallurgy and the Chemistry of Metals

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Q1) Cast iron as it is prepared in a blast furnace is a product of high purity.

A)True

B)False

Q2) According to the band theory, which of these statements provide(s) an explanation for the high electrical conductivity of metals

I. a partly filled conduction band

II. a valence band overlapping an empty conduction band

III. a filled valence band

IV. a large gap between the valence band and the conduction band

A) I and II

B) I and III

C) III

D) III and IV

E) IV

Q3) The following depicts a correctly balanced chemical equation illustrating roasting.2ZnS + 3O₂ \(\rarr\) 2ZnO + 2SO₂

A)True

B)False

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23

Chapter 22: Nonmetallic Elements and Their Compounds

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Q1) In which of the following compounds is sulfur in a positive oxidation state

A) H₂S

B) S₈

C) CaS

D) MnS

E) SO₃

Q2) Which one of the following compounds can react with water to form hydrogen gas

A) PCl₅

B) NO₂

C) H₂O₂

D) KH

E) NH₃

Q3) The following accurately depicts the balanced chemical equation for a laboratory preparation of nitrogen gas.NH₄NO₂(s) \(\rarr\) 2H₂O(g) + N₂(g)

A)True

B)False

Q4) Alkali metal hydrides are very reactive with water, forming H₂ gas.

A)True

B)False

Page 24

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Chapter 23: Transition Metals Chemistry and Coordination Compounds

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Q1) The best name for K₄[FeCl₂(CN)₄] is

A) tetrapotassium dichlorodicyanoiron(II).

B) potassium dichlorodicyanoiron(II).

C) potassium dichlorodicyanoferrate(III).

D) tetrapotassium dichlorobis(cyano)iron(III).

E) potassium dichlorotetracyanoferrate(II).

Q2) How many geometric isomers are possible for the complex [CrF₃Br₃]^3-

A) None, only one structure is possible

B) Two

C) Three

D) Four

E) None of the above

Q3) What is the oxidation number of Co in the complex Co(H₂O)₃Cl₃

A) +1

B) +2

C) +3

D) +4

E) None of the above

Page 25

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Chapter 24: Organic Chemistry

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Q1) Select the one molecule that is a saturated hydrocarbon.

A) C₂H₄

B) C₄H₈

C) C₄H₆

D) C₄H₁₀

E) C₄H₂

Q2) Cycloalkanes have the general formula

A) C_nH_2n-4.

B) C_nH_2n-2.

C) C_nH_2n.

D) C_nH_2n+2.

E) C_nH_2n+4.

Q3) Alkynes have the general formula

A) C_nH_2n-4.

B) C_nH_2n-2.

C) C_nH_2n.

D) C_nH_2n+2.

E) C_nH_2n+4.

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Chapter 25: Synthetic and Natural Organic Polymers

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Q1) A protein that has been reversibly denatured has

A) temporarily lost part or all of its secondary or tertiary structure.

B) temporarily lost part or all of its primary structure.

C) been genetically modified due to errors in the nucleotides in the parent DNA.

D) temporarily lost its amino acid residues.

E) temporarily lost the hydrogen bonding between nitrogenous bases.

Q2) Which of these molecules is a product of the hydrolysis of DNA

A) acetic acid

B) glucose

C) adenine

D) ribose

E) water

Q3) An amino acid is a compound that contains at least

A) one amino group and one amide group.

B) two amino groups and one carboxylic acid group.

C) one hydroxyl group and one methyl group.

D) one carboxylic acid group and one amino group.

E) one methyl group and one amide group.

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