Untitled Quiz

Study Notes

Density formula: d = m/V (density equals mass divided by volume).
Temperature conversion: C + 273 = K (Celsius to Kelvin).
Molarity formula: M = moles/liter (molarity is moles of solute per liter of solution).

Percent yield formula: (actual yield/theoretical yield) x 100 (measures efficiency of a reaction).
Percent composition formula: (molar mass of element/molar mass of compound) x 100 (calculates proportion of an element in a compound).
Boyle's Law: P1V1 = P2V2 (pressure-volume relationship in a gas).
Charles' Law: V1/T1 = V2/T2 (volume-temperature relationship in a gas).
Ideal Gas Equation: PV = nRT (relationship between pressure, volume, moles, gas constant, and temperature).
Combined Gas Law: P1V1/T1 = P2V2/T2 (combination of Boyle's and Charles' laws).
Gay-Lussac's Law: P1/T1 = P2/T2 (pressure-temperature relationship in a gas).

Heat capacity formula: C = ms (heat capacity equals mass times specific heat).
Heat change with specific heat: q = msΔt (heat change equals mass times specific heat and temperature change).
Heat change with heat capacity: q = CΔt (heat change equals heat capacity times temperature change).
Standard enthalpy of reaction: ΔH°(rxn) = ΣnΔH°f(products) - ΣnΔH°f(reactants) (calculates enthalpy change from formation enthalpies).
Enthalpy change from bond energy: ΔH° = ΣBE(reactants) - ΣBE(products) (calculates enthalpy change from bond energies).

Formal charges formula: (valence electrons) - (lone pairs) - 0.5(bonding electrons) = F.C. (determines charge on an atom in a molecule).
Dipole moment: μ = Q x r (dipole moment equals charge times distance between charges).
Bond order formula: 0.5(electrons in bonding orbitals - electrons in antibonding orbitals) (determines bond strength).

Rate expression: rate = -Δ[A]/ΔT = +Δ[B]/ΔT (describes the change in concentration over time).
Average rate: [ ]f - [ ]i / Tf - Ti (calculates the average rate of reaction).
Rate law: k = [A]^x[B]^y (relationship between concentration and rate of reaction).
First order rate law: rate = k[A] (first order dependence on reactant concentration).
First order integrated rate law: ln[A] = -kT + ln[A]o (describes concentration change over time).

Overall reaction order: x + y (sum of the powers in the rate law).
First order half-life: T1/2 = 0.693/k (time required for concentration to halve).
Second order rate law: rate = k[A]^2 (rate is dependent on the square of concentration).
Second order half-life: T1/2 = 1/k[A]o (specific to second order reactions).

Equilibrium concentration formula: Kc = products/reactants (calculates equilibrium constant for concentrations).
Equilibrium pressure formula: Kp = products/reactants (calculates equilibrium constant for pressures).
pH formula: pH = -log[H+] (calculates acidity).
pOH formula: pOH = -log[OH-] (calculates basicity).
Relationship: pH + pOH = 14.00 (sum of pH and pOH in aqueous solutions).
Ion-product constant of water: Kw = [H+][OH-] = 1.0 x 10^-14 (product of hydrogen and hydroxide ion concentrations).

Percent ionization formula: (ionized acid concentration at equilibrium / initial acid concentration) x 100 (measures strength of acid).
Relationship of Ka and Kb: (Ka)(Kb) = Kw (relationship between strengths of acids and bases).
Henderson-Hasselbalch Equation: pH = pKa + log([conjugate base]/[acid]) (calculates pH based on weak acid/basics ratio).