CHEM 219 MODULES 1–8 EXAMS & FINAL EXAM
– PRINCIPLES OF ORGANIC CHEMISTRY
(2026/2027) | PORTAGE LEARNING – VERIFIED
Q&A WITH CORRECT COMPLETE SOLUTION
|ALREADY GRADED A+
1. If a solution is prepared by dissolving 0.5 moles of sodium chloride (NaCl)
in 1 liter of water, what would be the expected effect on the boiling point of
the solution compared to pure water?
The boiling point will decrease due to the presence of the solute.
The boiling point will remain the same as pure water.
The boiling point will increase due to the colligative properties of
the solute.
The boiling point will increase, but only if the solution is heated.
2. Which of the following resources is NOT mentioned as a recommended
study aid for Chem 132 exam preparation?
Textbooks
Lecture notes
Online tutorials
Review sessions
3. Explain the significance of dynamic equilibrium in a reversible chemical
reaction and how it relates to the concentrations of reactants and
products.
It indicates that reactants are completely converted to products.
It shows that the concentrations of reactants and products remain
,constant over time.
It means that the reaction has stopped.
It implies that products are favored over reactants.
,4. If you have a nonpolar solute, which of the following solvents would you
expect it to dissolve in best, based on the 'like dissolves like' principle?
Water
Ethanol
Hexane
Ammonia
5. Given the standard molar entropies of the reactants and products, how
would you determine if a reaction is likely to be spontaneous at a given
temperature based on the calculated ΔSo?
If ΔSo is positive, the reaction is always spontaneous regardless of
temperature.
If ΔSo is negative, the reaction is spontaneous at high temperatures
only.
If ΔSo is positive and the temperature is high, the reaction is likely
spontaneous.
If ΔSo is zero, the reaction will not occur.
6. Explain the difference between molarity and molality in terms of their
definitions and applications in solution chemistry.
Molarity is based on volume, while molality is based on mass.
Molarity is used for solid solutions, while molality is for liquid
solutions.
Molarity measures solute per liter of solution, while molality
measures solute per kilogram of solvent.
Molarity is temperature-dependent, while molality is not.
7. What is the principle behind the phrase 'like dissolves like' in chemistry?
Polar solvents dissolve polar solutes
, Nonpolar solvents dissolve ionic solutes
All solutes dissolve in any solvent
Ionic compounds cannot dissolve in water
8. Explain the significance of ΔG in determining the spontaneity of a reaction.
What does it imply if ΔG is zero?
It indicates that the reaction will proceed spontaneously.
It suggests that the reaction is at equilibrium.
It means the reaction is non-spontaneous.
It shows that the reaction requires energy input.
9. Which of the following statements about spontaneous reactions is correct
under the conditions of constant temperature and pressure?
A reaction with a positive ∆G will be spontaneous
All reactions with a positive ∆H will not be spontaneous.
All reactions in which ∆G is negative will be spontaneous.
All reactions in which ∆G is not equal to zero will be spontaneous.
None of the above
10. Which of the following best describes a ligand in coordination chemistry?
A molecule that donates electrons to form a bond with a metal
ion
A type of chemical reaction involving the transfer of protons
A solution that contains a high concentration of solute
A measure of the speed at which a chemical reaction occurs
11. Given a scenario where ice melts into water at 0°C, which of the following
statements best describes the entropy change during this phase
– PRINCIPLES OF ORGANIC CHEMISTRY
(2026/2027) | PORTAGE LEARNING – VERIFIED
Q&A WITH CORRECT COMPLETE SOLUTION
|ALREADY GRADED A+
1. If a solution is prepared by dissolving 0.5 moles of sodium chloride (NaCl)
in 1 liter of water, what would be the expected effect on the boiling point of
the solution compared to pure water?
The boiling point will decrease due to the presence of the solute.
The boiling point will remain the same as pure water.
The boiling point will increase due to the colligative properties of
the solute.
The boiling point will increase, but only if the solution is heated.
2. Which of the following resources is NOT mentioned as a recommended
study aid for Chem 132 exam preparation?
Textbooks
Lecture notes
Online tutorials
Review sessions
3. Explain the significance of dynamic equilibrium in a reversible chemical
reaction and how it relates to the concentrations of reactants and
products.
It indicates that reactants are completely converted to products.
It shows that the concentrations of reactants and products remain
,constant over time.
It means that the reaction has stopped.
It implies that products are favored over reactants.
,4. If you have a nonpolar solute, which of the following solvents would you
expect it to dissolve in best, based on the 'like dissolves like' principle?
Water
Ethanol
Hexane
Ammonia
5. Given the standard molar entropies of the reactants and products, how
would you determine if a reaction is likely to be spontaneous at a given
temperature based on the calculated ΔSo?
If ΔSo is positive, the reaction is always spontaneous regardless of
temperature.
If ΔSo is negative, the reaction is spontaneous at high temperatures
only.
If ΔSo is positive and the temperature is high, the reaction is likely
spontaneous.
If ΔSo is zero, the reaction will not occur.
6. Explain the difference between molarity and molality in terms of their
definitions and applications in solution chemistry.
Molarity is based on volume, while molality is based on mass.
Molarity is used for solid solutions, while molality is for liquid
solutions.
Molarity measures solute per liter of solution, while molality
measures solute per kilogram of solvent.
Molarity is temperature-dependent, while molality is not.
7. What is the principle behind the phrase 'like dissolves like' in chemistry?
Polar solvents dissolve polar solutes
, Nonpolar solvents dissolve ionic solutes
All solutes dissolve in any solvent
Ionic compounds cannot dissolve in water
8. Explain the significance of ΔG in determining the spontaneity of a reaction.
What does it imply if ΔG is zero?
It indicates that the reaction will proceed spontaneously.
It suggests that the reaction is at equilibrium.
It means the reaction is non-spontaneous.
It shows that the reaction requires energy input.
9. Which of the following statements about spontaneous reactions is correct
under the conditions of constant temperature and pressure?
A reaction with a positive ∆G will be spontaneous
All reactions with a positive ∆H will not be spontaneous.
All reactions in which ∆G is negative will be spontaneous.
All reactions in which ∆G is not equal to zero will be spontaneous.
None of the above
10. Which of the following best describes a ligand in coordination chemistry?
A molecule that donates electrons to form a bond with a metal
ion
A type of chemical reaction involving the transfer of protons
A solution that contains a high concentration of solute
A measure of the speed at which a chemical reaction occurs
11. Given a scenario where ice melts into water at 0°C, which of the following
statements best describes the entropy change during this phase
