CHEM 110 Final Exam| verified Questions and Answers | 2026/2027 Update
| 100% correct| graded a+!!!! | pass!!
On a heating curve, what do sloped and flat lines represent? _answer-Sloped lines are
temperature change.
Flat lines are the phase changes (temperature does not change)
Label the important triple point and critical point on a phase diagram. _answer-
What is the name of the phase change: liquid to solid? _answer-Freezing
What is the name of the phase change: gas to liquid? _answer-Condensation
What is the name of the phase change: Gas to solid? _answer-Deposition
What is the name of the phase change: solid to liquid? _answer-Melting
What is the name of the phase change: Liquid to gas? _answer-Vaporization
What is the name of the phase change: solid to gas _answer-Sublimation
Which of the phase changes are exothermic and why? _answer-Condensation,
freezing, and deposition.
IMFs are formed and energy of molecules is lower.
Which of the phase changes are endothermic and why? _answer-Vaporization, melting,
and sublimation.
IMFs are broken and energy of molecules is higher.
What equation is used for temperature changes? _answer-q = m⋅c⋅ΔT
If q > 0, its endothermic
If q < 0, its exothermic
What equation is used for phase changes? _answer-q = n⋅ΔH
What does the vapor pressure of a substance depend on? _answer-The IMFs between
the molecules and the temperature of the substance.
, How to determine the approximate vapor pressure? _answer-Strong IMFs mean small
vapor pressure, weak IMFs mean high vapor pressure.
Describe the 2 major trends in viscosity. _answer-Viscosity increases as IMFs increase.
Viscosity decreases as temperature increases.
Describe the only major trend with surface tension. _answer-Surface tension increases
as IMFs increase.
What are the energy changes associated with dissolution process? _answer-1. Break
solvent-solvent interactions (requires energy, endothermic)
2. Break solute-solute interactions (requires energy, endothermic)
3. Form solute-solvent interactions (releases energy, exothermic)
What is an electrolyte? _answer-They ionize or dissociate in solution, and conduct an
electrical current.
What is a strong electrolyte? _answer-One that completely dissociates into ions.
Ionic compounds, strong acids, and strong bases.
What is a weak electrolyte? _answer-One that partially dissociates into ions.
Weak acids and weak bases.
What are non-electrolyes? _answer-Does not dissociate at all.
How to calculate M (molarity)? _answer-
When calculating dilutions, how would you find the moles of a solute? _answer-Molarity
times Volume.
How would you calculate a dilution? _answer-
How does the solubility of gases in water change with increasing temperature?
_answer-Solubility decreases with increasing temperature.
How does the solubility of gases change with increasing pressure? _answer-Solubility
increases with increasing pressure.
How does the solubility of solids change with increasing temperature? _answer-
Solubility increases with increasing temperature.
What is Henry's law and what does it solve for? _answer-Solubility of a gas (C).
C = Henry's Law Constant⋅Pgas
What is the rule of thumb for solubility rules? _answer-Polar solvents tend to dissolve
polar and ionic solutes.
| 100% correct| graded a+!!!! | pass!!
On a heating curve, what do sloped and flat lines represent? _answer-Sloped lines are
temperature change.
Flat lines are the phase changes (temperature does not change)
Label the important triple point and critical point on a phase diagram. _answer-
What is the name of the phase change: liquid to solid? _answer-Freezing
What is the name of the phase change: gas to liquid? _answer-Condensation
What is the name of the phase change: Gas to solid? _answer-Deposition
What is the name of the phase change: solid to liquid? _answer-Melting
What is the name of the phase change: Liquid to gas? _answer-Vaporization
What is the name of the phase change: solid to gas _answer-Sublimation
Which of the phase changes are exothermic and why? _answer-Condensation,
freezing, and deposition.
IMFs are formed and energy of molecules is lower.
Which of the phase changes are endothermic and why? _answer-Vaporization, melting,
and sublimation.
IMFs are broken and energy of molecules is higher.
What equation is used for temperature changes? _answer-q = m⋅c⋅ΔT
If q > 0, its endothermic
If q < 0, its exothermic
What equation is used for phase changes? _answer-q = n⋅ΔH
What does the vapor pressure of a substance depend on? _answer-The IMFs between
the molecules and the temperature of the substance.
, How to determine the approximate vapor pressure? _answer-Strong IMFs mean small
vapor pressure, weak IMFs mean high vapor pressure.
Describe the 2 major trends in viscosity. _answer-Viscosity increases as IMFs increase.
Viscosity decreases as temperature increases.
Describe the only major trend with surface tension. _answer-Surface tension increases
as IMFs increase.
What are the energy changes associated with dissolution process? _answer-1. Break
solvent-solvent interactions (requires energy, endothermic)
2. Break solute-solute interactions (requires energy, endothermic)
3. Form solute-solvent interactions (releases energy, exothermic)
What is an electrolyte? _answer-They ionize or dissociate in solution, and conduct an
electrical current.
What is a strong electrolyte? _answer-One that completely dissociates into ions.
Ionic compounds, strong acids, and strong bases.
What is a weak electrolyte? _answer-One that partially dissociates into ions.
Weak acids and weak bases.
What are non-electrolyes? _answer-Does not dissociate at all.
How to calculate M (molarity)? _answer-
When calculating dilutions, how would you find the moles of a solute? _answer-Molarity
times Volume.
How would you calculate a dilution? _answer-
How does the solubility of gases in water change with increasing temperature?
_answer-Solubility decreases with increasing temperature.
How does the solubility of gases change with increasing pressure? _answer-Solubility
increases with increasing pressure.
How does the solubility of solids change with increasing temperature? _answer-
Solubility increases with increasing temperature.
What is Henry's law and what does it solve for? _answer-Solubility of a gas (C).
C = Henry's Law Constant⋅Pgas
What is the rule of thumb for solubility rules? _answer-Polar solvents tend to dissolve
polar and ionic solutes.
