Upgrade to remove ads
Only $35.99/year

Chemistry Semester 2 Test

Terms in this set (78)

Mole (Chapter 7)
SI unit that measures the amount of substance (mol)
Moles to atoms (Chapter 7)
Avogadro's number (6.02 x 10^23 = 1 mole)
Atoms to moles (Chapter 7)
1 mole = 6.02 x 10^23 (Avogadro's number)
Moles to liters (Chapter 7)
1 mol = 22.4L
Avogadro's number (Chapter 7)
6.02 x 10^23
Standard temperature and pressure (Chapter 7)
- (STP)
- Zero degrees Celcius
- 101.3 kPA
- (Molar volume = 22.4 L at STP)
7 diatomic molecules (Chapter 7)
- Hydrogen
- Nitrogen
- Oxygen
- Fluorine
- Chlorine
- Iodine
- Bromine
Balancing equations (Chapter 8)
1) Write the correct formula for each reactant and product
2) Working with one atom, adjust coefficients to balance that atom. If a polyatomic is the same on both sides, balance as a unit
3) Do H's and O's last if possible
4) Reduce coefficients if possible
Chemical equations (Chapter 8)
Describe chemical reactions
Chemical equation symbols (Chapter 8)
(+): Used to separate one reactant or product from another
(-->): Used to separate the reactants from the products - "Yields/produces"
(g): Indicates that the substance is in a gaseous state
(s): Indicates that the substance is in a solid state
(l): Indicates that the substance is in a liquid state
(aq): Indicates that the substance is dissolved in water (aqueous)
(Triangle): Heat is used
Chemical reactions (Chapter 8)
Produce new substances/matter
Conservation of Mass (Chapter 8)
Chemical equations must be balanced to satisfy this law
Limiting Reactant (Chapter 8)
- Reactant that is used up first in a chemical equation
- Determines the amount of produce that can be formed in the reaction
Stoichiometry (Chapter 9)
The calculation of quantities in a chemical reaction
Stoichiometry steps (Chapter 9)
1) Balanced equation
2) Convert given (G) to moles
3) Mole ratio
4) Moles to wanted (W)
Sets with similar terms