Name______

Date______

Period______

A#______

Final Review

Equations:

C to K, Gas laws, specific heat, molarity, ∆Hr, ∆G, pH, pOH

Classify each reaction by type, then balance. Finally, write a word equation for each.

1. Al + O2  Al2O3 ______

2. Ca(OH)2 + HNO3  Ca(NO3)2 + H2O ______

3. Cu + AgNO3  Cu(NO3)2 + Ag ______

4. PbO2  PbO + O2 ______

Name the followingWrite formulas for the following

  1. PCl ______9. sulfuric acid______
  2. N2O4______10. hydrofluoric acid ______
  3. H2S ______11. ammonium phosphate ______
  4. H2CO3______12. diphosphorus pentoxide_____

Stoichiometry

  1. How many moles of carbon dioxide are produced from the combustion of 100.g of methane (CH4)?
  1. How many grams of hydrogen are produced if 80. g of water reacts completely? 2Na + 2H2O → 2NaOH + H2
  1. What volume of NH3 at STP is produced if 25.0g of N2 is reacted with an excess of hydrogen gas? N2 + 3H2 →2NH3
  1. Determine the number of atoms in 25g of NaCl.

Solve

  1. How much heat would be absorbed by 75g of iron when heated from 295K to 301K?
  1. Calculate the change in enthalpy for the following reaction.

FeO(s) + O2(g) → 2Fe2O3(s)

  1. When graphite reacts with hydrogen at 300K, the change in enthalpy is -74.8 kJ/mol and entropy change is -.0809 kJ/mol K. Will this reaction occur spontaneously?
  1. Predict if value of S will be >, <, or =to 0, and give reason why.

3H2(g) + N2(g) →2NH3(g)

C6H12O6(s) + 6O2(g) →6CO2(g) + 6H2(g)

  1. How many grams of KNO3 should be used to prepare 2.00L of a .500M solution?
  1. A 180.0mL volume of gas is measured at 87.0°C. If the pressure remains unchanged, what is the volume of the gas at standard temperature?
  1. The volume of a sample of oxygen is 300.0 mL when the pressure is 1 atm and the temperature is 27.0C. At what temperature is the volume 1.00L and the pressure 0.500atm?
  1. A 425 mL sample of gas is collected at 780. mm Hg. If the temperature remains constant and the pressure falls to 680. mm Hg, what is the new volume?
  1. Calculate the mass of hydrogen peroxide needed to obtain .460L of oxygen gas at STP. 2H2O2(aq) → 2H2O + O2(g)
  1. What are the different phase transitions? Label each as endo. or exothermic.
  1. What factors affect reaction rates?
  1. Label the energy diagram.

Acids & Bases

  1. What are properties of acids and bases?
  1. pgs. 883-884 #’s 1-27 odd

List of topics:

  1. Chemical Equations
  2. chemical formulas - empirical vs. molecular formula
  3. types of reactions/classifying
  4. balancing equations
  5. Stoichiometry/ conversions
  6. molar ratios
  7. g→ mol
  8. g→g
  9. Avogadro’s #
  10. Thermodynamics
  11. Specific heat
  12. Calorimetry
  13. Enthalpy of reaction – endo. vs. exo.
  14. Spontaneity – Gibb’s Free Energy
  15. Phase transitions – endo.vs. exo.

f. Energy diagrams – activation energy for forward and reverse, reactants, products, etc.

  1. Gas Laws
  2. all laws and whether direct or inverse relationship between variables
  3. STP
  4. Absolute zero
  5. Avogadro’s Law 22.4L/1mol at STP
  6. Reaction Rates/Equilibrium

a. factors affecting

  1. Acid/Bases
  2. SolutionspH scaleneutralizationtitration
  3. MolarityArrhenius/Bronsted Lowry acid/base
  4. PropertiesConjugatepH/pOH calculations