CHEM 1128. ACS Final Exam Practice 2 LATEST
VERSION-2023 WITH 100% CORRECT
RATIONALE. VERIFIED&GRADED A+
Condensed States of Matter - ANSWER solids and liquids, molecules are close
enough to interact with each other
Strong Intramolecular Force - ANSWER occurs within molecule (covalent and ionic
bonding)
Weak Intramolecular Force - ANSWER attraction forces between atoms in dif.
molcules
-hydrogen bonds
-london dispersion forces
-dipole induced dipole forces
Dipole-Dipole Forces - ANSWER a polarized molecules w/ partially pos. and neg.
poles
strength of force decreases as distance between dipoles increase
(only in polar covalent compounds)
Hydrogen Bonds - ANSWER special type of dipole-dipole force but. much stronger
form when H+ (pos. end) attract to N, O, or F- (partially neg.)
Measurement of Vapor Pressure - ANSWER Pvapor = P atmosphere - P Hg
column
Vapor Pressure & IMFS - ANSWER -strong IMF = low vapor pressure
-weak IMF = high vapor pressure
Enthalpy of Vaporization - ANSWER ln(Pvap) = (-∆Hvap / R) (1/T) + C
T- temp K
∆Hvap- enthalpy of vaporization
R- univ gas constant
C- constant of given liquid
Clausius-Clapeyron Equation - ANSWER shows relationship between VP, temp,
and ∆Hvap
ln (Pvap, T1/Pval T2) = (∆Hvap / R) (1/T2- 1/T1)
solution - ANSWER homogenous mixture of 2 or more substances
Solute - ANSWER component that is being dissolved
Solvent - ANSWER compound that is doing the dissolving
, Molarity (M) - ANSWER mols of solute (mol) / volume solution (L)
Molality (m) - ANSWER moles of solute (mol) / mass of solvent (kg)
Mole fraction - ANSWER moles of component A (mol) / total # moles of all
components (mol)
Mass Percent (weight %) - ANSWER (mass of solute / mass of solution) x 100%
Factors Affecting Solubility - ANSWER structure, temperature, and pressure
Structure Effects - ANSWER if 2 substances have similar IMF, likely to be soluble in
one another
-nonpolar solvents dissolve nonpolar solutes
-polar solvents dissolve polar solutes
Pressure Effects - ANSWER pressure increases solubility of gas
-Henry's Law
Henry's Law - ANSWER the amount of a gas dissolved in a solution is directly
proportional to the pressure of the gas above the solution
Cg = kPg
Cg- solubility of gas
Pg= partial pressure of gas
k- proportionally constant
Temp Effects (aqueous solutions) - ANSWER solids dissolve rapidly at higher
temps
solubility can decrease with increasing temp
Temp Effects (for gas) - ANSWER solubility of gas in water decreases w/
increasing temp
Colligative Properties - ANSWER depend only on total conc. of solute species
regardless of indentities
Non-electrolyte - ANSWER compounds that doe not dissociate into ions
Roult's Law - ANSWER Pa = XaPa°
Pa- partial pressure exerted by solvent when a non-volatile solute is dissolved
Xa- mole fraction of A in solution
Pa°- vapor pressure of solvent A
Boiling Point Elevation - ANSWER ∆Tb = Kbm
∆Tb- change in BP / BP elevation
Kb- BPE constant
m- molality of solute (mol/kg)
Freezing Point Depression - ANSWER ∆Tf = Kfm
∆Tf- freezing point depression
VERSION-2023 WITH 100% CORRECT
RATIONALE. VERIFIED&GRADED A+
Condensed States of Matter - ANSWER solids and liquids, molecules are close
enough to interact with each other
Strong Intramolecular Force - ANSWER occurs within molecule (covalent and ionic
bonding)
Weak Intramolecular Force - ANSWER attraction forces between atoms in dif.
molcules
-hydrogen bonds
-london dispersion forces
-dipole induced dipole forces
Dipole-Dipole Forces - ANSWER a polarized molecules w/ partially pos. and neg.
poles
strength of force decreases as distance between dipoles increase
(only in polar covalent compounds)
Hydrogen Bonds - ANSWER special type of dipole-dipole force but. much stronger
form when H+ (pos. end) attract to N, O, or F- (partially neg.)
Measurement of Vapor Pressure - ANSWER Pvapor = P atmosphere - P Hg
column
Vapor Pressure & IMFS - ANSWER -strong IMF = low vapor pressure
-weak IMF = high vapor pressure
Enthalpy of Vaporization - ANSWER ln(Pvap) = (-∆Hvap / R) (1/T) + C
T- temp K
∆Hvap- enthalpy of vaporization
R- univ gas constant
C- constant of given liquid
Clausius-Clapeyron Equation - ANSWER shows relationship between VP, temp,
and ∆Hvap
ln (Pvap, T1/Pval T2) = (∆Hvap / R) (1/T2- 1/T1)
solution - ANSWER homogenous mixture of 2 or more substances
Solute - ANSWER component that is being dissolved
Solvent - ANSWER compound that is doing the dissolving
, Molarity (M) - ANSWER mols of solute (mol) / volume solution (L)
Molality (m) - ANSWER moles of solute (mol) / mass of solvent (kg)
Mole fraction - ANSWER moles of component A (mol) / total # moles of all
components (mol)
Mass Percent (weight %) - ANSWER (mass of solute / mass of solution) x 100%
Factors Affecting Solubility - ANSWER structure, temperature, and pressure
Structure Effects - ANSWER if 2 substances have similar IMF, likely to be soluble in
one another
-nonpolar solvents dissolve nonpolar solutes
-polar solvents dissolve polar solutes
Pressure Effects - ANSWER pressure increases solubility of gas
-Henry's Law
Henry's Law - ANSWER the amount of a gas dissolved in a solution is directly
proportional to the pressure of the gas above the solution
Cg = kPg
Cg- solubility of gas
Pg= partial pressure of gas
k- proportionally constant
Temp Effects (aqueous solutions) - ANSWER solids dissolve rapidly at higher
temps
solubility can decrease with increasing temp
Temp Effects (for gas) - ANSWER solubility of gas in water decreases w/
increasing temp
Colligative Properties - ANSWER depend only on total conc. of solute species
regardless of indentities
Non-electrolyte - ANSWER compounds that doe not dissociate into ions
Roult's Law - ANSWER Pa = XaPa°
Pa- partial pressure exerted by solvent when a non-volatile solute is dissolved
Xa- mole fraction of A in solution
Pa°- vapor pressure of solvent A
Boiling Point Elevation - ANSWER ∆Tb = Kbm
∆Tb- change in BP / BP elevation
Kb- BPE constant
m- molality of solute (mol/kg)
Freezing Point Depression - ANSWER ∆Tf = Kfm
∆Tf- freezing point depression
