Rice CHEM 122 Formula/Info Sheet Cheat Sheet (DRAFT) by kaliap714

Formula Name	Equation
Boyle's Law	PV = k (N,T)
Charles's Law	V/T = k (N,P)
Avogadro's Law	V/n = k (T,P)
Ideal Gas Law	V = nRT/P or PV = nRT
Dalton's Law	Ptotal = P1 + P2 + P3....
STP	1 atm, 0 Celsius
Gas Density	d = m/V = PM/RT = N/V
Partial Pressure	P1 = X1 * Ptotal
Root Mean Squared Speed	v = sqrt(3­RT/M)
Collision Frequency	f = vrms / mfp (mean free path)
Average Kinetic Energy	KE = 3/2 nRT
Effusion - Graham's Law	rate1/­rate2 = sqrt(M­W2/MW1)
General Rate Law	rate = k[A]m*[B]n
Zeroth Order Integrated Rate Law	[A]t = [A]0 - kt
First Order Integrated Rate Law	ln[A]t = ln[A]0 -kt
Second Order Integrated Rate LAw	1/[A]t = 1/[A]0 + kt
Zeroth Order Half Life	t = [A]0/2k
First Order Half Life	t = ln2/k
Second Order Half Life	t = 1/k[A]0
Arrhenius Equation	Ae^-Ea/RT
Logari­thmic Form of Arrhenius Equation	ln(k2/k1) = (-Ea/R) * (1/T2 - 1/T1)
Michae­lis­-Menton Enzyme Kinetics	rate = k2 [E]T [S]/[S] + km

Formula Name/S­ubject	Equati­on/­Des­cri­ption
Equili­brium Constant (conce­ntr­ations)	Kc = [produ­cts­]/[­rea­ctants]
Equili­brium Constant (press­ures)	Kp = P(prod­uct­s)/­P(r­eac­tants)
Equili­brium Equation (with rates)	K = kf/kr
Q = K	At equili­birum
Q < K	reaction shifts in forward direction
Q > K	reaction shifts in reverse direction
Keq is large (10^3)	kforward > kreverse
Keq is small (10^-3)	kforward < kreverse
Keq = 1	kforward = kreverse
Kc and Kp Relation	Kc = Kp * RT^Δn
L'C: add more reactants	reaction shifts forward
L'C: add more products	reaction shifts reverse
L'C: increase pressure	reaction shifts towards fewer moles
L'C: decrease pressure	reaction shifts towards greter moles
L'C: increase volume	reaction shifts towards greater moles
L'C: decrease volume	reaction shifts towards fewer moles
Endoth­ermic (T) Phase Transi­tions	Melting, Sublim­ation, Evapor­ation
Exothermic (P) Phase Transi­tions	Freezing, Deposi­tion, Conden­sation
Entropy	S = kB ln(W)
Change in Entropy for Change in Volume	ΔS = nR ln(V2/V1)
Change in Entropy ofSurr­oun­dings	ΔSsurr = -ΔH/T
Gibbs Free Energy	ΔG = ΔH - TΔS
Nonsta­ndard Gibbs Free Energy (1)	ΔG = ΔG0 + RTlnQ
Standard Gibbs Free Energy	ΔG0 = -RTlnK
Nonsta­ndard Gibbs Free Energy (2)	ΔG = RT ln(Q/K)
Clausi­sus­-Cl­aperyon Equation	ln(P2/P1) = -ΔH/R (1/T2-­1/T1)

Formula Name/Info	Equati­on/­Des­cri­ption
Molarity (M)	mol solute/L solution (mol/L)
Molality (m)	mol solute/kg solution (mol/kg)
Mole Fraction (X)	mol solute/mol solution (mol/mol)
Vapor Pressure (two volatile chemicals)	Pvap = PaXa + PbXb
Boiling Point Elevation	Tb = kb m i
Freezing Point Depression	Tf = -kf m i
Osmotic Pressure	pi =iMRT
Solubility	S = mol dissolved / L solution
CIE: add in species already present	decrease solubility
Hender­son­-Ha­sse­lbach Equation	pH = pKa + log(conj. base/acid)
K value for Neutra­liz­ation	Kn = Ka*Kb/Kw
Equiva­lence Point	mol base added = mol acid originally present
Midpoint	pH = pKa
Solven­t-S­olvent Intera­ctions	endoth­ermic, overcome IMFs
Solute­-Solute Intera­ctions	endoth­ermic, overcome IMFs
Solven­t-S­olute Intera­ctions	exothe­rmic, release energy through attractive forces
To relate Ka to Kb	Kw = Ka * Kb
Strong Acids	H2SO4, HNO3, HCl, HI, HClO4, HClO3, HBr
Strong Bases	LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2

Formula Name/S­ubject	Equati­on/­Des­cri­ption
Current (I))	charge­/time (Amperes)
Voltage (V)	energy­/charge (Volts)
Power (W)	energy­/se­conds (Watts)
Oxidation Reaction	Lose electrons
Reduction Reaction	Gain electrons
Cathode	Site of reduction, e- flow to cathode
Anode	Site of oxidation, e- flow from anode
Cell Potential (E)	Ecell = Ecathode + Eanode = Eredcat - Eredan
Gibbs Free Energy (standard)	ΔG0 = -nFE0
Faraday's Constant	96,500 C/mol e-
Nernst Equation	E = E0 - RT/nF lnQ
Standard Hydrogen Electrode (SHE)	2H+ + 2e- -> H2(g)
Standard Cell Potential	E0 = RT/nF lnK
Total Charge (Z)	Z = I * t (in seconds), in coloumbs
Moles of Electrons Produced	n(e-) = Z/F
Moles of Metal Produced	n(metal) = n(e-)* mol(me­tal­)/mols e- needed
Mass of Metal Produced	m(metal) = n(meta­l)/­MWmetal
Nernst Equation with pH	E = E0red + 2.3RT/F logQ