Download Chemistry 111: Exam 1 Topics

Chemistry 111: Exam 3 Topics
Chapter 9
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Mass calculations
(massmolesmolesmass)
You will have the map on the exam
cover sheet!
Find % yield
Use % yield as a conversion factor
Find limiting reagents
Chapter 4
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Understand kinetic theory – explain
pressure/temp/volume based on
molecular collisions
Understand how to read a barometer
Understand how to read a manometer
Be able to convert pressure units
Remember to use Kelvin!
Understand what’s held constant in
Boyle’s Law, Charles’ Law
Use combined gas law
(P1V1/T1=P2V2/T2 is given).
Chapter 15: Gases, Liquids & Solids
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Chapter 16: Solutions
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Chapter 13: Ideal Gas Law
(PV=nRT)
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Recognize that you have to solve this type of
problem – should have 4 out of 5 gas
variables.
Set up a table to solve the problem!
Be able to use equation for gas density.
Use n=PV/RT for stoichoimetry (ugh)
Sometimes cheat - @ STP have 22.4 L/mol
of any gas
Partial Pressure
Intermolecular Forces (IMF)
o Dipole-Dipole
o London Dispersion (Induced Dipole)
o Hydrogen Bond
o Figure 15.9!
Know viscosity, boiling point, Hvap,
surface tension, vapor pressure.
Relate the above to IMF
Types of solids – what holds them together
(ionic bond, covalent bond, or IMF?)
Calculate heat for temperature changes.
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Vocabulary
Formation of a solution – NaCl  hydrated
Na+ & ClIMF & Solubility
Concentration Units
o % (g/100g)
o ppm (mg/L)
o Molarity (mol/L)
Dilution (M1V1=M2V2)
Solution Stoichiometry – Conc (M) 
Volume (L) = moles
Titration (2 cases only):
o Easy – 1:1 stoichiometry, M1V1=M2V2
o Lab: 1:1 stoich, find MW
Also: Know the lab calculations / concepts for the short-answer part of the exam.