Title | Chemistry Formula Sheet |
---|---|
Course | General Chemistry I |
Institution | University of Guelph |
Pages | 5 |
File Size | 161.9 KB |
File Type | |
Total Downloads | 45 |
Total Views | 156 |
This is a basic refresher for the students that lack some knowledge in the CHEM1040 department...
``Important Chemistry Formulas/Guide from Grade 11-12 Converting Metric Units Sheet Metric Prefixes
Numerical values
Written Notation
Tera
Unit value x1012
T
Giga
Unit value x109
G
Mega
Unit value x106
M
Kilo
Unit value x103
k
Hecto
Unit value x102
h
Deca
Unit value x101
da
Baseline
1 meter or whatever unit of measurement we are using
None
Deci
Unit value x10-1
d
Centi
Unit value x10-2
c
Milli
Unit value x10-3
m
Micro
Unit value x10-6
� (pronounced mu)
Nano
Unit value x10-9
n
Pico
Unit value x10-12
p
Femto
Unit value x1015
f
Important conversion tips for chemistry
Temperature Celsius to Fahrenheit
FT=
Celsius to Kelvin
KT=CT+273.15
Gas Conversions Atmosphere to mmhg/torr
1 atm = 760mmhg/torr
Atmosphere to kilopascals
1 atm = 101.3kPa
Bar to Atmosphere
1 atm = 1.01325 bar
Important Chemical Formulas
Stoichiometric Formulas
Gaseous Formulas
m=MMn
Force =
Mass of 1 atom/molecule=
Pressure =
Mass % in compounds =
Boyle’s Law
Molecular formula =
Charles's Law =
How to get empirical formula
Combined Gas Law =
*** this must be done for each element Ideal Gas Law = in compound Gas density = Percentage yield =
Molar Concentration (Molarity) = Chemical Equilibrium
Acids and Bases
A mixture of 1 mole of carbon monoxide and 3 moles of hydrogen gas are placed in a 10.0L vessel at 1200K and are brought to equilibrium. Find the amount of products produced in an equilibrium given the following equation.
Key Strong Acids: HClO4, H2SO4, HI, HBr, HCl, HNO3
Start values: 1.0 mol, 3.00 mol ? Change: -x -3x +x Equilibrium: 1.0mol-x
3.0mol-3x
x
Key Strong Bases: LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 Self Ionization of Water: Kw=[H3O+][OH-]=1.0x10-14 at 25℃
? pH/pOH of a solution: +x x=0.387
pH = -log [H3O+] pOH = -log [OH-]
Solve for the other compounds
pH + pOH = 14.00
Kc Equilibrium Constant
Acid ionization Constant Ka
Take this equation for example aA+bB ⇆ cC dD
Ka =
Kc =
*** PRODUCTS OVER REACTANTS
*** PRODUCTS OVER REACTANTS The Reaction Quotient Qc
Qc = If Qc is > Kc then the equilibrium shifts left to the reactants (Too much product is made or too little reactants is left) If Qc is < Kc then the equilibrium shifts right to the products (Not enough product is made or too much reactant left) If Qc = Kc then the reaction is at
Polyprotic acids: Acids that can donate more than one hydrogen ion H2SO4 Gotta calculate Ka1 and Ka2 Base Ionization constant Kb Kb = pH of a salt solution:
equilibrium Ka Kb = Kw Remember Le Chatelier’s Principle in an equilibrium if any changes are done Henderson-Hasselbalch Equation: that would disturb the equilibrium. The pH = pKa + log reaction will act in an attempt to reverse the effects and restore equilibrium Organic Chemistry Guide
Other Equations:
Hydrocarbon prefixes: Meth-1 Eth-2 Prop-3 But-4 Penta-5 Hexa-6 Hepta-7 Octa-8 Nona-9 Deca-10
c
Functional Groups: Hydroxyl (OH) Carbonyl (=O) Carboxyl (=O +OH) Phenyl (Benzene ring) Amino (NH2) Nitro (NO2) Ether (R’-O-R) R means carbon chain O ⇈ Ester (R’-C-O-R) *Ignore arrows they represent a double bond O ⇈ Amide (R-C-NH-R’)
Ɛ=h*ν E = NA * Ɛ
Variable Guide: MM = MOLAR MASS (g/mol) m = mass (g) n = moles (mol) C = Celsius F = Fahrenheit K = Kelvin P = Pressure T = Temperature V = Volume D = density d = gas density Avogadro’s # = 6.02x1023 R = Molar gas constant (0.082058 L·atm/(K·mol)) c = speed of light in a vacuum 3.0e8 ms-1 Ɛ = Energy of one photon E = One Mole of Quantized energy ƛ = wavelength ν = frequency h = Planck’s Constant (6.626x10-34J*s)...