Stoichiometry (Chapter 9, Pg 250), Definition, A Branch of Chemistry where quantities in chemical reactions are calculated., Mole-Mole Calculations, Examples, Mass-Mass Calculations, Examples, 9.1 The Arithmetic of equations, 9.2 Chemical Calculations
Chemical Quantities (Chapter 7, Pg 189), 7.1 The mole: A measurement of matter, 7.2 Mole-mass and Mole- volume relationships, 7.3 Percentage Composition and chemical formulas, Definition, The percent by mass of each element in a compound., Formula, %Mass of element = (Grams of element/grams of compound) * (100/1), Using the Formula:
States of Matter (Chapter 10, Pg), 10.1 The nature of gases, 10.2 The nature of liquids, 10.3 The nature of solids, 10.4 Changes of state
The Behavior of Gases (Chapter 12, Pg), 12.1 The properties of gases, 12.2 Factors affecting gas pressure, 12.3 The gas laws, Boyles Law, Charles Law, Gays Law, 12.4 Ideal gases, 12.5 Gas molecules: Mixtures and Movements
Reaction Rates and Equilibrium (Chapter 19, Pg 544), Equilibrium, What can alter Equilibrium?, Pressure, Concentration, Temperature, Catalyst, Although can effect changes such as pressure we say there's no effect when a catalyst is added., 19.1, 19.2, 19.3
Acids and Bases (Chapter 20, Pg), 20.1, 20.2, 20.3, 20.4
Neutralization (Chapter 21, Pg), 21.2, New node
D = (M/V), Density = (Molar Mass/Volume)
n = (N/Na), Mole = (Representative Particles/Avogadro's Number)
n = (m/M), Mole = (Mass/Molar Mass)
nRT = PV, New node
n = (V/Vo), Mole = (Volume/Molar Volume), (P1V1/T1)=(P2V2/T2), (Pressure1*Volume1/Temperature1)=(Pressure2*Volume2/Temperature2)
Using the Formulas:, n = (N/Na), Eg: How many moles of Pb is 9.3*10^15 atoms of Pb? n = (9.3*10^15 / 6.02*10^23) n = 1.5*10^-8 mol, D = (M/V), Eg:, n = (m/M), Eg: How many moles of CO2 is 12.3 grams of CO2? n = (12.3g / 44g/mol) n = 0.279mol, n = (V/Vo), Eg:
Avogadro's Number, 6.02*10^23, Symbol - Na
Mole, The amount of a substance that contains 6.02*10^23 representative particles of a substance., Symbol - n
Gram atomic Mass (gam), The atomic mass of an element expressed in grams.
Gram Formula Mass (gfm), Formula mass of an ionic substance expressed in grams.
Gram Molecular Mass (gmm), The mass of one mole of a molecular compound.
Representative Particle, The atoms, molecules, or ions present in a substance., Symbol - N
Molar Mass, Mass (in grams) of one mole of a substance., Symbol - M
STP, Standard Temperature and Pressure
Molar Volume, 22.4 L of gas at STP, Symbol - Vo
Percentage Composition, The percent by mass of each element in a compound.
Empirical Formula, The lowest whole-number ratio of atoms of the elements in a compound.
Molecular Formula, Describes the actual number of atoms of each element in a molecule of a compound.
Standard Pressure, 101.3 kPa or 1 atm
Molar Road Map, A mean of relating mass, numbr of particles, and gaseous volume of a substance.
Standard Temperature, 0 oC or 273 K
Stoichiometry, A branch of chemistry where quantities in chemical reactions are calculated.
Kinetic Theory, New node
Kinetic Energy, New node
Amorphous, New node
Unit cell, New node
Crystal, New node
Normal Boiling Point, New node
Barometer, New node
atmospheric pressure, New node
melting point, New node
Sublimination, New node
Boiling point, New node
Allotrope, New node
Vapor pressure, New node
Evaporation, New node
Supercooled Liquid, New node
Collision Theory, New node
Chemical Equilibrium, New node
Le Chateliers Principle, New node
Molar Mass, M (g/mol)
Mass, m (grams)
Mole, n (mol)
Density, New node
Molar Volume, Vo (22.4 L)
Avogadro's Number, Na (6.02*10^23)
Volume, V (L)
Representative Particles, N
Universal Gas, R (8.31)