chem quizlet

Gibbs free energy change equation

∆G = -nFEcell

Equilibrium Constant (Kc)

Kc = [C]^c[D]^d / [A]^a[B]^b

Polarity of Molecules

A molecule with polar bonds may be polar or nonpolar depending on the orientation of the bond dipoles.

PV = k or P1V1 = P2V2

Boyle's Law relating pressure and volume of a gas.

V/T = k or V1/T1 = V2/T2

Charles's Law relating volume and temperature of a gas.

P/T = k or P1/T1 = P2/T2

Gay-Lussac's Law relating pressure and temperature of a gas.

(P + a)(V - nb) = nRT

Van der Waals equation of state accounting for real gas behavior.

PV = nRT

Ideal Gas Law relating pressure, volume, temperature, and moles of gas.

q = mc∆T

Formula for heat transfer where q is heat, m is mass, c is specific heat, and ∆T is temperature change.

1 mole of gas at STP = 22.4 L

Volume of one mole of an ideal gas at standard temperature and pressure.

PA = PTXA

Dalton's law of partial pressures relating total pressure and partial pressures.

Enthalpy (H)

Is used to express heat changes at constant pressure.

Kinetic molecular theory of gases

An explanation of gaseous molecular behavior based on the motion of individual molecules.

Average molecular speeds

K = 1/2 mv² = 3/2 kBT

Standard heat of formation (∆H°f)

The enthalpy change that would occur if one mole of a compound was formed directly from its elements in their standard states.

Standard heat of reaction (∆H°rxn)

The hypothetical enthalpy change that would occur if the reaction were carried out under standard conditions.

Root-mean-square speed (urms)

urms = √(3RT/M)

Hess's law

States that enthalpies of reactions are additive.

Entropy (S)

The measure of the distribution of energy ('randomness') throughout a system.

Gibbs free energy (G)

Combines the two factors that affect the spontaneity of a reaction—changes in enthalpy, ∆H, and changes in entropy, ∆S.

Gibbs free energy equation

∆G = ∆H - T∆S

Colligative properties

Physical properties derived solely from the number of particles present, not the nature of those particles.

Freezing point depression equation

∆Tf = iKfm

Boiling point elevation equation

∆Tb = iKbm

Osmotic pressure equation

∏ = MRT

pH equation

pH = -log[H+] = log(1/[H+])

pOH equation

pOH = -log[OH-] = log(1/[OH-])

Kw equation

Kw = [H+][OH-] = 10-14

pH + pOH equation

pH + pOH = 14

Ka equation

Ka = [H3O+][A-]/[HA]

Kb equation

Kb = [B+][OH-]/[BOH]

Percent composition by mass

Mass of solute / Mass of solution × 100%

Molarity equation

# of mol of solute / liter of solution

Molality equation

# of mol of solute / kg of solvent

Normality equation

# of gram equivalent weights of solute / liter of solution

Henderson-Hasselbalch equation

pH = pKa + log [conjugate base] / [weak acid]

Standard reduction potential equation

emf = E˚red, cathode - E˚red, anode

Moles

Moles = mass of a sample / molar mass

Avogadro's Number

A mole is represented by Avogadro's number, 6.022 x 10^23 particles.

Rate Law Equation

rate = k[A]^x[B]^y

Energy of Electron

E = Hn

Electromagnetic Energy of Photons

E = hc

Maximum Number of Electrons in Energy Level

Maximum number of electrons = 2n²

Formal Charge

Formal charge is the charge an atom would have if all the electrons in bonds were shared equally.

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