% composition
mass element/mass compound x 100
molecular formula
(empirical formula) x (X)
1 mol (avagadros #)
6.02 x 10^23
1 mol (gas at STP)
22.4 L
% yield
actual yield/theoretical yield x 100
Grahams Law
Rate A/Rate B = square of Ma/Mb
Daltons Law
total pressure = P1+P2+P3..
Boyles Law
P1V1=P2V2
Charles Law
V1T1 = V2T2
Gay Lusacs Law
P1T1 = P2V2
Combined Gas Law
P1V1/T1 = P2V2/T2
Ideal Gas Law
PV = nRT
Density of a Gas
Density = MP/RT
Molar mass of a Gas
M = mRT/PV
Standard Temperature
1 atm at 0 degrees
Standard Pressure
101.3 kPa at 273 K
Standard Molar Volume (gas at STP)
22.4 L = 1 mol
Standard Temp & Pressure
1 atm = 101.3 kpa
Henrys Law
S1/P1 = S2/P2
Percent by mass (m/m)
mass solute/mass solution x 100
Percent by volume (v/v)
volume solute/volume solution x 100
Molarity (M)
mole solute/liters solution
Molality (m)
mole solute/kg solvent
Mole fraction
mole solute/mole solute + mole solvent
Dilution equation
M1V1 = M2V2
Freezing point depression
Tf = Kf x m x i
Boiling point elevation
Tb = Kb x m x i
energy equation
(Hrxn)(# moles)
H*rxn
H
r(products) - H
r(reactants)
Gsystem
Hsystem - Tsystem
q
(m)(c)(t)
1 Calorie
1 kcal
1 kcal
1000 calories
1000 calories
1 Calorie
Average Reaction Rates
concentration/time
rate
k[A]m[B]n
aA + bB
cC + dD
Keq
[C]c[D]d/[A]a[B]b
Keq >
products favored
Keq <
reactants favored
AaBb(s)
aA(aq) + bB(aq)
Ksp
[A]a[B]b
Qsp < Ksp
no precipitate
Qsp > Ksp
precipitate
pH
-log[H+]
pOH
-log[OH-]
[H+]
antilog(-pH)
[OH-]
antilog(-pOH)
pH + pOH
14
[H+] x [OH-]
1 x 10^-14
Keq of weak acid
Ka
Keq of weak base
Kb
Titrations
M1V1 = M2V2
Mole ratio
Moles A = Moles B
Molar Mass
Mass A (g) = 1 mole A
Acogadros #
particles A = 1 mole A
Molar Volume
liters A = 1 mole A