GENERAL CHEMISTRY II EXAM – QUESTIONS AND ANSWERS | VERIFIED AND WELL
DETAILED ANSWERS | PLUS RATIONALES | GUARANTEED PASS | LATEST EXAM UPDATE
Core Domains: Intermolecular Forces and Liquids Properties of Solutions Chemical Kinetics
Chemical Equilibrium Acids and Bases Aqueous Equilibria Chemical Thermodynamics
Electrochemistry
Introduction: The purpose of this comprehensive examination is to rigorously evaluate
advanced mastery of core chemical principles and quantitative problem-solving
methodologies. The assessment measures critical skills in analyzing molecular interactions,
reaction rates, equilibrium systems, thermodynamic favorability, and electrochemical cell
potentials. Utilizing a balanced mixture of traditional multiple-choice questions and complex
scenario-based assessments, this test evaluates analytical reasoning rather than rote
memorization. Particular emphasis is placed on real-world applications in laboratory and
industrial settings, empowering candidates to make scientifically sound decisions,
troubleshoot chemical phenomena, and apply foundational theory to complex practical
dilemmas.
Section One: Questions 1–100
Question 1 Which of the following substances exhibits hydrogen bonding as its primary
intermolecular force in the pure liquid state? A. H2S B. CH4 C. NH3 D. PH3 C. NH3
Explanation: Hydrogen bonding occurs when hydrogen is covalently bonded to highly
electronegative atoms such as nitrogen, oxygen, or fluorine. Ammonia contains N-H bonds,
whereas the other options exhibit weaker dipole-dipole or London dispersion forces.
Question 2 What is the primary factor responsible for the high boiling point of water
compared to other group 16 hydrides like H2Se and H2S? A. Molecular weight B. Extensive
hydrogen bonding network C. Linear molecular geometry D. High polarizability of oxygen
B. Extensive hydrogen bonding network Explanation: Water molecules can form an
extensive, multi-directional network of hydrogen bonds due to the small size and high
electronegativity of oxygen, requiring significantly more thermal energy to separate
molecules into the gas phase.
Question 3 Which phase transition is exothermic? A. Melting B. Vaporization C. Sublimation
D. Condensation D. Condensation Explanation: Condensation involves transitioning
from a high-energy gas to a lower-energy liquid state, releasing heat to the surroundings,
making the process exothermic.
Question 4 What is the name of the temperature and pressure point on a phase diagram
where all three phases of a substance coexist in equilibrium? A. Critical point B. Triple point
C. Boiling point D. Fusion point B. Critical point Explanation: The triple point on a
phase diagram represents the unique combination of temperature and pressure where solid,
liquid, and gas phases exist simultaneously in dynamic equilibrium.
,Question 5 Which unit of concentration is temperature-dependent because it involves the
volume of the solution? A. Molality B. Mole fraction C. Molarity D. Mass percentage C.
Molarity Explanation: Molarity is defined as moles of solute per liter of solution. Because
solution volume changes slightly with temperature due to thermal expansion or contraction,
molarity is temperature-dependent.
Question 6 According to Henry's Law, the solubility of a gas in a liquid is directly proportional
to which of the following? A. Temperature of the liquid B. Partial pressure of the gas above
the liquid C. Volume of the container D. Molar mass of the gas B. Partial pressure of the
gas above the liquid Explanation: Henry's law states that at a constant temperature, the
solubility of a given gas is directly proportional to the partial pressure of that gas maintained
in contact with the liquid.
Question 7 Which of the following aqueous solutions would be expected to have the lowest
freezing point? A. 0.10 m NaCl B. 0.10 m C6H12O6 C. 0.10 m MgCl2 D. 0.10 m AlCl3 D.
0.10 m AlCl3 Explanation: Freezing point depression is a colligative property dependent
on the total concentration of particles in solution. Aluminum chloride dissociates into four
ions (Al3+ and 3 Cl-), yielding the highest particle concentration and lowest freezing point.
Question 8 What term describes the scattering of light by colloidal particles in a mixture? A.
Diffraction B. Tyndall effect C. Osmosis D. Refraction B. Tyndall effect Explanation:
The Tyndall effect is the phenomenon where light passing through a colloid is scattered by
the dispersed particles, making the light beam visible through the mixture.
Question 9 For a zero-order reaction, what is the unit of the rate constant (k)? A. s-1 B. M s-1
C. M-1 s-1 D. M-2 s-1 B. M s-1 Explanation: Rate equals the rate constant for a zero-
order reaction (Rate = k). Because rate has units of concentration per time (M/s or M s-1),
the rate constant must share these units.
Question 10 If the half-life of a first-order reaction is independent of the initial concentration
of the reactant, what is the half-life of a reaction with a rate constant of 0.0693 s-1? A. 5.0 s
B. 10.0 s C. 20.0 s D. 69.3 s B. 10.0 s Explanation: For a first-order reaction, the half-
life is calculated using the formula t1/2 = 0.693 / k. Substituting the given rate constant: t1/2
= 0..0693 s-1 = 10.0 s.
Question 11 Which factor does a catalyst alter to increase the rate of a chemical reaction? A.
Enthalpy change of the reaction B. Activation energy C. Equilibrium constant D. Gibbs free
energy of formation B. Activation energy Explanation: A catalyst provides an
alternative reaction pathway with a lower activation energy, thereby increasing the rate of
both the forward and reverse reactions without changing the overall thermodynamics.
Question 12 In the Arrhenius equation, k = A exp(-Ea / RT), what does the symbol A
represent? A. Activation energy B. Universal gas constant C. Frequency factor D. Rate
, constant C. Frequency factor Explanation: The symbol A represents the frequency
factor, which is related to the frequency of collisions and the orientation probability of the
reactant molecules.
Question 13 What is the molecularity of an elementary reaction step that involves three
reactant molecules colliding simultaneously? A. Unimolecular B. Bimolecular C. Termolecular
D. Quadmolecular C. Termolecular Explanation: Molecularity refers to the number of
reactant particles coming together in an elementary step. A step involving three colliding
particles is termed termolecular.
Question 14 For a reversible reaction at chemical equilibrium, which of the following
statements is true? A. The rates of the forward and reverse reactions are equal. B. The
concentrations of reactants and products are equal. C. The reaction has stopped completely.
D. The forward rate constant equals the reverse rate constant. A. The rates of the
forward and reverse reactions are equal. Explanation: Chemical equilibrium is a dynamic
state where the rate of the forward reaction equals the rate of the reverse reaction, resulting
in constant macroscopic concentrations over time.
Question 15 Write the expression for the equilibrium constant, Kc, for the reaction: 2SO2(g)
+ O2(g) <=> 2SO3(g). A. [SO3]^2 / ([SO2]^2 [O2]) B. ([SO2]^2 [O2]) / [SO3]^2 C. [SO3] /
([SO2] [O2]) D. ([SO2] [O2]) / [SO3] A. [SO3]^2 / ([SO2]^2 [O2]) Explanation: The
equilibrium constant expression is formulated as the product of product concentrations
raised to their stoichiometric coefficients divided by the product of reactant concentrations
raised to their coefficients.
Question 16 If the reaction quotient (Qc) is greater than the equilibrium constant (Kc) for a
given system, what will happen? A. The reaction will proceed in the forward direction. B. The
reaction is already at equilibrium. C. The reaction will proceed in the reverse direction. D.
The rate of the forward reaction will increase. C. The reaction will proceed in the reverse
direction. Explanation: When Qc > Kc, there is an excess of products relative to
reactants. The system will shift to the left (reverse direction) to consume products and re-
establish equilibrium.
Question 17 According to Le Chatelier's principle, how will an endothermic equilibrium
system respond to an increase in temperature? A. Shift in the forward direction to absorb
added heat B. Shift in the reverse direction to produce heat C. Experience no shift in
equilibrium position D. Decrease the value of the equilibrium constant A. Shift in the
forward direction to absorb added heat Explanation: An endothermic reaction absorbs
heat. Increasing the temperature imposes a stress that the system relieves by shifting in the
direction that consumes heat, which is the forward direction.
DETAILED ANSWERS | PLUS RATIONALES | GUARANTEED PASS | LATEST EXAM UPDATE
Core Domains: Intermolecular Forces and Liquids Properties of Solutions Chemical Kinetics
Chemical Equilibrium Acids and Bases Aqueous Equilibria Chemical Thermodynamics
Electrochemistry
Introduction: The purpose of this comprehensive examination is to rigorously evaluate
advanced mastery of core chemical principles and quantitative problem-solving
methodologies. The assessment measures critical skills in analyzing molecular interactions,
reaction rates, equilibrium systems, thermodynamic favorability, and electrochemical cell
potentials. Utilizing a balanced mixture of traditional multiple-choice questions and complex
scenario-based assessments, this test evaluates analytical reasoning rather than rote
memorization. Particular emphasis is placed on real-world applications in laboratory and
industrial settings, empowering candidates to make scientifically sound decisions,
troubleshoot chemical phenomena, and apply foundational theory to complex practical
dilemmas.
Section One: Questions 1–100
Question 1 Which of the following substances exhibits hydrogen bonding as its primary
intermolecular force in the pure liquid state? A. H2S B. CH4 C. NH3 D. PH3 C. NH3
Explanation: Hydrogen bonding occurs when hydrogen is covalently bonded to highly
electronegative atoms such as nitrogen, oxygen, or fluorine. Ammonia contains N-H bonds,
whereas the other options exhibit weaker dipole-dipole or London dispersion forces.
Question 2 What is the primary factor responsible for the high boiling point of water
compared to other group 16 hydrides like H2Se and H2S? A. Molecular weight B. Extensive
hydrogen bonding network C. Linear molecular geometry D. High polarizability of oxygen
B. Extensive hydrogen bonding network Explanation: Water molecules can form an
extensive, multi-directional network of hydrogen bonds due to the small size and high
electronegativity of oxygen, requiring significantly more thermal energy to separate
molecules into the gas phase.
Question 3 Which phase transition is exothermic? A. Melting B. Vaporization C. Sublimation
D. Condensation D. Condensation Explanation: Condensation involves transitioning
from a high-energy gas to a lower-energy liquid state, releasing heat to the surroundings,
making the process exothermic.
Question 4 What is the name of the temperature and pressure point on a phase diagram
where all three phases of a substance coexist in equilibrium? A. Critical point B. Triple point
C. Boiling point D. Fusion point B. Critical point Explanation: The triple point on a
phase diagram represents the unique combination of temperature and pressure where solid,
liquid, and gas phases exist simultaneously in dynamic equilibrium.
,Question 5 Which unit of concentration is temperature-dependent because it involves the
volume of the solution? A. Molality B. Mole fraction C. Molarity D. Mass percentage C.
Molarity Explanation: Molarity is defined as moles of solute per liter of solution. Because
solution volume changes slightly with temperature due to thermal expansion or contraction,
molarity is temperature-dependent.
Question 6 According to Henry's Law, the solubility of a gas in a liquid is directly proportional
to which of the following? A. Temperature of the liquid B. Partial pressure of the gas above
the liquid C. Volume of the container D. Molar mass of the gas B. Partial pressure of the
gas above the liquid Explanation: Henry's law states that at a constant temperature, the
solubility of a given gas is directly proportional to the partial pressure of that gas maintained
in contact with the liquid.
Question 7 Which of the following aqueous solutions would be expected to have the lowest
freezing point? A. 0.10 m NaCl B. 0.10 m C6H12O6 C. 0.10 m MgCl2 D. 0.10 m AlCl3 D.
0.10 m AlCl3 Explanation: Freezing point depression is a colligative property dependent
on the total concentration of particles in solution. Aluminum chloride dissociates into four
ions (Al3+ and 3 Cl-), yielding the highest particle concentration and lowest freezing point.
Question 8 What term describes the scattering of light by colloidal particles in a mixture? A.
Diffraction B. Tyndall effect C. Osmosis D. Refraction B. Tyndall effect Explanation:
The Tyndall effect is the phenomenon where light passing through a colloid is scattered by
the dispersed particles, making the light beam visible through the mixture.
Question 9 For a zero-order reaction, what is the unit of the rate constant (k)? A. s-1 B. M s-1
C. M-1 s-1 D. M-2 s-1 B. M s-1 Explanation: Rate equals the rate constant for a zero-
order reaction (Rate = k). Because rate has units of concentration per time (M/s or M s-1),
the rate constant must share these units.
Question 10 If the half-life of a first-order reaction is independent of the initial concentration
of the reactant, what is the half-life of a reaction with a rate constant of 0.0693 s-1? A. 5.0 s
B. 10.0 s C. 20.0 s D. 69.3 s B. 10.0 s Explanation: For a first-order reaction, the half-
life is calculated using the formula t1/2 = 0.693 / k. Substituting the given rate constant: t1/2
= 0..0693 s-1 = 10.0 s.
Question 11 Which factor does a catalyst alter to increase the rate of a chemical reaction? A.
Enthalpy change of the reaction B. Activation energy C. Equilibrium constant D. Gibbs free
energy of formation B. Activation energy Explanation: A catalyst provides an
alternative reaction pathway with a lower activation energy, thereby increasing the rate of
both the forward and reverse reactions without changing the overall thermodynamics.
Question 12 In the Arrhenius equation, k = A exp(-Ea / RT), what does the symbol A
represent? A. Activation energy B. Universal gas constant C. Frequency factor D. Rate
, constant C. Frequency factor Explanation: The symbol A represents the frequency
factor, which is related to the frequency of collisions and the orientation probability of the
reactant molecules.
Question 13 What is the molecularity of an elementary reaction step that involves three
reactant molecules colliding simultaneously? A. Unimolecular B. Bimolecular C. Termolecular
D. Quadmolecular C. Termolecular Explanation: Molecularity refers to the number of
reactant particles coming together in an elementary step. A step involving three colliding
particles is termed termolecular.
Question 14 For a reversible reaction at chemical equilibrium, which of the following
statements is true? A. The rates of the forward and reverse reactions are equal. B. The
concentrations of reactants and products are equal. C. The reaction has stopped completely.
D. The forward rate constant equals the reverse rate constant. A. The rates of the
forward and reverse reactions are equal. Explanation: Chemical equilibrium is a dynamic
state where the rate of the forward reaction equals the rate of the reverse reaction, resulting
in constant macroscopic concentrations over time.
Question 15 Write the expression for the equilibrium constant, Kc, for the reaction: 2SO2(g)
+ O2(g) <=> 2SO3(g). A. [SO3]^2 / ([SO2]^2 [O2]) B. ([SO2]^2 [O2]) / [SO3]^2 C. [SO3] /
([SO2] [O2]) D. ([SO2] [O2]) / [SO3] A. [SO3]^2 / ([SO2]^2 [O2]) Explanation: The
equilibrium constant expression is formulated as the product of product concentrations
raised to their stoichiometric coefficients divided by the product of reactant concentrations
raised to their coefficients.
Question 16 If the reaction quotient (Qc) is greater than the equilibrium constant (Kc) for a
given system, what will happen? A. The reaction will proceed in the forward direction. B. The
reaction is already at equilibrium. C. The reaction will proceed in the reverse direction. D.
The rate of the forward reaction will increase. C. The reaction will proceed in the reverse
direction. Explanation: When Qc > Kc, there is an excess of products relative to
reactants. The system will shift to the left (reverse direction) to consume products and re-
establish equilibrium.
Question 17 According to Le Chatelier's principle, how will an endothermic equilibrium
system respond to an increase in temperature? A. Shift in the forward direction to absorb
added heat B. Shift in the reverse direction to produce heat C. Experience no shift in
equilibrium position D. Decrease the value of the equilibrium constant A. Shift in the
forward direction to absorb added heat Explanation: An endothermic reaction absorbs
heat. Increasing the temperature imposes a stress that the system relieves by shifting in the
direction that consumes heat, which is the forward direction.
