1. Semester II Review

2. Semester I Review Give the formula for the following compounds
1) iron (II) arsenide Fe3As2
2) lead (II) sulfate PbSO4
3) lead (IV) hydroxide Pb(OH)4
4) copper (II) acetate Cu(C2H3O2)2
5) beryllium chloride BeCl2
6) ammonium chromate (NH4)2CrO4
7) silver oxide Ag2O
8) potassium sulfide K2S

3. Semester I Review Give the name of the following compounds
1) NaBr Sodium Bromide
2) Sc(OH)3 Scandium (III) Hydroxide
3) V2(SO4)3 Vanadium (III) Sulfate
4) NH4F Ammonium Fluoride
5) CaCO3 Calcium Carbonate
6) NiPO4 Nickel (III) Phosphate
7) Li2SO3 Lithium Sulfite
8) Zn3P2 Zinc Phosphide
9) Sr(C2H3O2)2 Strontium Acetate
10) Cu2O Copper (I) Oxide

4. SM II Review Name the compounds H2SO3 Sulfurous Acid
H2S Hydrosulfuric acid
H3PO4 Phosphoric acid
HCN Hydrocyanic acid
H3P Hydrophosphoric acid
HBr Hydrobromic acid
HClO Hypochlorous acid

5. SM II Review Give the formula for the following compounds
hydrofluoric acid HF
hydroselenic acid H2Se
carbonic acid H2CO3
nitrous acid HNO2
sulfuric acid H2SO4
hydrobromic acid HBr
Chlorous acid HClO2

6. SM II Review Antimony tribromide SbBr3 Silicon difluoride SiF2
Tetracarbon octahydride C4H8
Dinitrogen monoxide N2O
Pentaphosphorous decoxide P5O10
Sulfur hexachloride SF6

7. SM II Review P2O5 Diphosphorous pentoxide SO2 Sulfur dioxide
NO2 Nitrogen dioxide
AsCl3 Arsenic trichloride
P4H8 Tetraphosphorous octahydride

8. Semester I Review Balance and classify the reactions
_2_ C8H18 + _25_ O2  _16_ CO2 + _18_ H2O
____ FeCl3 + _3__ NaOH  ____ Fe(OH)3 + _3__NaCl
_4__ P + __5_O2  _2__P2O5
_2__ Na + _2__ H2O  __2_ NaOH + ____H2
_2__ Ag2O  _4__ Ag + ____O2
____ S8 + _12_ O2  _8__ SO3

9. SM II Review
For a given chemical reaction, the theoretical yield is generally more than the actual yield
The first step in most stoichiometry problems is to balance the equation.

10. SM II Review
Hydrogen gas reacts with nitrogen gas to form ammonia gas.
Write and balance the equation
3H N2  2NH3
Determine the Limiting reactant if 3.50 g of hydrogen reacts with 42.0 g of nitrogen.
What is the theoretical yield of the above problem? g NH3
What is the % yield if the reaction produced 15.3 g of ammonia %
Calculate the amount of grams of excess reactant leftover at the end of the reaction 25.8 g N2 Leftover

11. SM II Review
What is the empirical formula of a compound that is % Na, % S, and % O. Na2SO4
If the molecular formula molar mass is , what is the molecular formula of the above compound. Na4S2O8
What is the percent composition of FeO? % Fe and 22.27% O

12. SM II Review
Calculate the specific heat of an unknown metal, given that 25.0g of the metal lost 3570 J of energy during a temperature change from 100.0oC to 25.0oC
c = -3570J / (25.0g)x(-75.0oC)
c = 1.90 J/goC

13. SM II Review
Identify each of the letters on the graph and explain what is occurring.
C = solid warming/cooling
D = Phase change solid to liquid or vice versa
E = liquid warming/cooling
F = phase change liquid to gas or vice versa
G = gas warming/cooling C D E F G

14. SM II Review Label the solid, liquid, and gas regions on the graph.
Label the triple point and critical point
At 600oC and 90 atm, what phase is yummygum in? Liquid
Critical point
liquid
solid
Triple point
gas

15. SM II Review
Calculate the amount of heat released if 25.0g of steam is cooled from oC to (-15.0 oC)
Phase 1 q = (25.0g)(2.01J/goC)(100oC -150oC) = J
Phase change q = (25.0g)(-2260J/g) = J
Phase 2 q = (25.0g)(4.184J/goC)(0oC-100 C) = J
Phase change q = (25.0g)(-334J/g) = J
Phase 3 q = (25.0g)(2.03J/goC)(-15oC – 0 oC) = J
Total Energy = J

16. SM II Review
If the volume of a container holding a gas is reduced, what will happen to the pressure within the container? Increase
What happens to the temperature of a gas when it is compressed? Increases
What happens to the pressure of a gas inside a container, if the temperature of the gas is lowered? Decreases
The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change? Decreases by 2 times

17. SM II Review Boyle’s law states that PV = K, inverse proportion.
Charles’ law states that V/T = K, direct proportion.
Gay-Lussac’s law states that P/T = K, direct proportion.
Avogadro’s law states that V/n = K, direct proportion.
Dalton's Law states that sum of all the pressures = the total pressure.

18. SM II Review
A gas confined in a 305 mL container exerts a pressure of 1.07 atm at 38.6°C. At what Celsius temperature will it exert a pressure of 2.75 atm if it is placed into a 644 mL container?
1506 K = 1233 °C

19. SM II Review
What is the pressure inside a 3.0 L flask if 30.5 g of Carbon Monoxide is held at a temperature of oC?
11 atm or 1100 kPa