ACS CHEMISTRY ACTUAL EXAMINATION 2025/2026
QUESTIONS WITH SOLUTIONS GRADED A+
✔✔How do you determine polarity? - ✔✔Use the chart that has electronegativity values,
then subtract the elements in the compound from each other.
✔✔Is water polar? - ✔✔Yes!
✔✔Combination Reaction? - ✔✔A + B --> AB
✔✔Decomposition Reaction? - ✔✔AB --> A + B
✔✔Single Replacement Reaction? - ✔✔AB + C --> AC + B
✔✔Double Replacement Reaction? - ✔✔AB + CD --> AD + CB
✔✔Combustion Reaction? - ✔✔C + H + O --> H2O + CO2 always
✔✔Avogadro's Number? - ✔✔6.022 x 10^23 particles = 1 mole
✔✔Molar Mass? - ✔✔gram/mole
✔✔Mole to Volume? - ✔✔1 mole = 22.4 L
✔✔Empirical Formula vs Molecular Formula? - ✔✔Molecular = the actual number of
atoms in a compound
Empirical = basic ratio, smallest whole numbers of atoms in a compound
✔✔Percent Composition? - ✔✔Mass element/mass compound x 100
✔✔Limiting Reactant? - ✔✔The reactant which runs out first...meaning it limits how
much product can be made
ex: If there's 1 mole of NaOH and 2 moles of HCl, NaOH is the limiting reactant,
because it is used up (only 1 mole)
✔✔Which state of matter has the greatest Kinetic Energy? - ✔✔Gas has the greatest
KE, because the particles are far apart and moving fast
✔✔What are the three types of Intermolecular Forces? - ✔✔(1) Hydorgen Bonding
(2) Dipole Attraction
(3) Dispersion Forces
✔✔What do you call a solid changing to a gas? - ✔✔Sublimation
, ✔✔What are the values for STP? - ✔✔0 Celcius or 273 Kelvin
1 atm = 101.3 kPa = 760 mmHg
✔✔Why is the pressure of a gas directly proportional to the number of particles? -
✔✔P1/N1 = P2/N2....because pressure is caused by collisions of gas, and more
particles means more collisions
✔✔Why is the volume of a gas inversely proportional to pressure? - ✔✔P1 x V1 = P2 x
V2...because as volume increases, there is less opportunity for particles to collide
✔✔Why is the pressure of a gas directly proportional to temperature? - ✔✔P1/T1 =
P2/T2....because as temperature increases, KE increases, which makes collisions
happen more often and harder
✔✔Why is the volume of a gas directly proportional to temperature? - ✔✔V1/T1 =
V2/T2....because as temperature increases, KE increases, and the particles spread
aout
✔✔PV=nRT - ✔✔Pressure x Volume = # of moles x Gas Constant x Temperature
✔✔Dalton's Law of Partial Pressure? - ✔✔P total = P1 + P2 + P3 ...
✔✔Graham's Law of Effusion? - ✔✔Rate A/Rate B = Square Root of Molar Mass
B/Molar Mass A
✔✔If a solution is saturated, is there left over solute? - ✔✔Yes, saturated = left over
solute
Unsaturated = all solute is dissolved
✔✔Molarity (M)? - ✔✔Moles Solute mole
---------------- ------
Liters Solution L
✔✔Making Dilutions? - ✔✔M1V1 = M2V2
✔✔Percent By Mass? - ✔✔% m/m = mass solute
--------------- x 100
mass solution
✔✔molality (m)? - ✔✔Moles Solute mole
--------------- ---------
kg Solvent kg
✔✔Specific Heat? - ✔✔c = q/mΔT
QUESTIONS WITH SOLUTIONS GRADED A+
✔✔How do you determine polarity? - ✔✔Use the chart that has electronegativity values,
then subtract the elements in the compound from each other.
✔✔Is water polar? - ✔✔Yes!
✔✔Combination Reaction? - ✔✔A + B --> AB
✔✔Decomposition Reaction? - ✔✔AB --> A + B
✔✔Single Replacement Reaction? - ✔✔AB + C --> AC + B
✔✔Double Replacement Reaction? - ✔✔AB + CD --> AD + CB
✔✔Combustion Reaction? - ✔✔C + H + O --> H2O + CO2 always
✔✔Avogadro's Number? - ✔✔6.022 x 10^23 particles = 1 mole
✔✔Molar Mass? - ✔✔gram/mole
✔✔Mole to Volume? - ✔✔1 mole = 22.4 L
✔✔Empirical Formula vs Molecular Formula? - ✔✔Molecular = the actual number of
atoms in a compound
Empirical = basic ratio, smallest whole numbers of atoms in a compound
✔✔Percent Composition? - ✔✔Mass element/mass compound x 100
✔✔Limiting Reactant? - ✔✔The reactant which runs out first...meaning it limits how
much product can be made
ex: If there's 1 mole of NaOH and 2 moles of HCl, NaOH is the limiting reactant,
because it is used up (only 1 mole)
✔✔Which state of matter has the greatest Kinetic Energy? - ✔✔Gas has the greatest
KE, because the particles are far apart and moving fast
✔✔What are the three types of Intermolecular Forces? - ✔✔(1) Hydorgen Bonding
(2) Dipole Attraction
(3) Dispersion Forces
✔✔What do you call a solid changing to a gas? - ✔✔Sublimation
, ✔✔What are the values for STP? - ✔✔0 Celcius or 273 Kelvin
1 atm = 101.3 kPa = 760 mmHg
✔✔Why is the pressure of a gas directly proportional to the number of particles? -
✔✔P1/N1 = P2/N2....because pressure is caused by collisions of gas, and more
particles means more collisions
✔✔Why is the volume of a gas inversely proportional to pressure? - ✔✔P1 x V1 = P2 x
V2...because as volume increases, there is less opportunity for particles to collide
✔✔Why is the pressure of a gas directly proportional to temperature? - ✔✔P1/T1 =
P2/T2....because as temperature increases, KE increases, which makes collisions
happen more often and harder
✔✔Why is the volume of a gas directly proportional to temperature? - ✔✔V1/T1 =
V2/T2....because as temperature increases, KE increases, and the particles spread
aout
✔✔PV=nRT - ✔✔Pressure x Volume = # of moles x Gas Constant x Temperature
✔✔Dalton's Law of Partial Pressure? - ✔✔P total = P1 + P2 + P3 ...
✔✔Graham's Law of Effusion? - ✔✔Rate A/Rate B = Square Root of Molar Mass
B/Molar Mass A
✔✔If a solution is saturated, is there left over solute? - ✔✔Yes, saturated = left over
solute
Unsaturated = all solute is dissolved
✔✔Molarity (M)? - ✔✔Moles Solute mole
---------------- ------
Liters Solution L
✔✔Making Dilutions? - ✔✔M1V1 = M2V2
✔✔Percent By Mass? - ✔✔% m/m = mass solute
--------------- x 100
mass solution
✔✔molality (m)? - ✔✔Moles Solute mole
--------------- ---------
kg Solvent kg
✔✔Specific Heat? - ✔✔c = q/mΔT
