CHEM 1210 Lecture Notes - Lecture 4: Chemical Formula, Combined Gas Law, Carbon-12

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Published on 13 Oct 2016
CHEM 1210
Solids, Liquids, and Gases
I. States of Matter
a. Solids
i. particles are rigidly held together
ii. definite shape and volume
b. Liquids
i. Particles are free to slip past one another
ii. Definite volume
iii. Take shape of container
iv. Not easily compressed
c. Gases
i. Particles are VERY far apart
ii. Indefinite shape and volume
d. Phase Transitions
i. Solid to liquid= melting
ii. Liquid to gas= boiling
iii. Solid to gas= sublimation
iv. Gas to liquid= condensation
v. Liquid to solid= freezing
vi. Gas to solid= deposition
II. Temperature
a. 1.8(C) = (F) 32
b. K = (C) + 273.15
i. 0 K is absolute 0 (as cold as possible)
c. Common Temperature Conversions
i. Boiling Point of Water = 212 F = 100 C = 373 K
ii. Normal Body Temperature = 98.6 F = 37 C = 310 K
iii. Average Room Temperature = 75 F = 24 C = 297 K
iv. Freezing Point of Water = 32 F = 0 C = 273 K
III. Mole (mol)- SI unit for amount of substance
a. The amount of a sustae that otais as a foula uits (atos, oleules,
ions, etc..) as there are in exactly 12 g of carbon-12
1. Epeietall, this ue is eual to Avagado’s ue; 6.  23
a. Ex.1) 1 mole of Cu = 63.55g of copper = 6.02 x 1023 Cu atoms
b. Ex. 2) 1 mole of Al = 26.98g of aluminum = 6.02 x 1023 Al atoms
c. Ex. 3) 1 mol of MgCl2
Mg 24.31 x 1 = 24.31g
Cl 365.45 x 2 = 70.90 24.31g + 70.90 = 95.21g
IV. Molar Mass = mass (in grams) of 1 mol of a substance
a. Add up the average atomic masses of all the atoms in the chemical formula
ii. Uses periodic table and chemical formula only
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