Review Unit

Molecular mass	Avogadro constant	Mole	Molar mass
Percentage composition	Ionic bond	Covalent bond	Anion
Cation	Chemical symbol	Chemical formula	Metal
Nonmetal	Metalloid

Equations Unit

Chemical reaction	reactant	product	single displacement	double displacement
decomposition	synthesis	combustion

Stoichiometry Unit

stoichiometry	percent yield	standard temperature	standard pressure	STP
limiting reactant	excess reactant	Avogadro’s principle	molar volume	ideal gas equation
combined gas law

State Standards Unit

atoms	Matter	Subatomic particle	Electron	Charged
Electron cloud	Nucleus	Electrostatic attraction	Proton	AMU
Neutron	Bohr model	energy levels	atomic number	atomic mass
elements	groups	periods	categories	Chemical properties
valence electrons	periodic table	metals	nonmetals	noble gases
transition elements	electron configuration	pattern (trends)	chemical bonds	molecules
energy	ionic compounds	cations	anions	covalent bonds
molecular compound	polar bonds	chemical formula	bond polarity	electron-dot diagram
chemical reaction	reactants	products	chemical equations	atoms
law of conservation of mass	stoichiometric relationships	balanced chemical equation	coefficient

Acid/Bases Unit

electrolyte	hydronium ion	conjugate base	conjugate acid	binary acid
binary acid	ternary acid	strong acid	strong base	weak acid
weak base	salt	neutralization reaction	spectator ion	polyprotic acid
pH	pH scale	pOH	indicator	titration
standard solution

Organic Unit

alkane	alkene	alkyne	radical	branch
substituent	saturated hydrocarbon	unsaturated hydrocarbon	alcohol	saponification

Final Review.

Stoichiometry

1. In a very violent reaction called a thermite reaction, aluminum metal reacts with iron (III) oxide to form iron metal and aluminum oxide.

a. Write a balanced chemical equation for this reaction.

b. What mass of Al will react with 150 g of iron (III) oxide?

c. If 0.905 mol of aluminum oxide is produced in the reaction, what mass of iron is produced?

d. How many moles of iron (III) oxide will react with 99. grams of aluminum?

2. Acetaldehyde, CH₃CHO, is manufactured by the reaction of ethanol with copper (II) oxide according to the following equation:

CH₃CH₂OH + CuO à CH₃CHO + H₂O + Cu

a. What mass of acetaldehyde can be produced by the reaction between 620 g of ethanol and 1020 g of CuO? What mass of which reactant will be left over?

b. If this is a 48.6% yield reaction how much acetaldehyde is actually produced?

3. Calculate the percent yield in each of the following cases.

a. Theoretical yield is 50. g of product; actual yield is 41.9 g

b. Theoretical yield is 290 kg of product; actual yield is 270 kg

c. 68.3 g of ethyl acetate should be produced but only 43.9 are recovered.

d. 0.0419 mol of ethyl acetate is produce but 0.0722 mol is expected.

4. Methanol, CH₃OH, is frequently used in race cars as fuel. It is produced as the sole product of the synthesis reaction from carbon monoxide gas and hydrogen gas.

a. If 430 kg of hydrogen react, what mass of methanol could be produced?

b. If the reaction is a 52 percent yield reaction, what mass is actually produced?

Solutions

5. Water is a polar solvent, do polar or nonpolar solutes dissolve better? Why?

6. If 28g of KNO₃ is dissolved in 230 ml what is the molarity of the solution?

7. DON’T DO

8. How many grams of NaNO₃ are dissolved in 275 ml of a .500 M solution?

9. How many grams of K₂CrO₄ are dissolved in 175 ml of a 1.84 M solution?

10. DON’T DO

11. What volume of .32M HCL would be required to react completely with 1.75 moles of NaOH?

12. What volume of 4.25 M HNO₃ solution would be required to completely react with 345 ml of a 2.00 M Ca(OH)₂?

13. What is the molarity of a H₃PO₄ solution if 135 ml are required to completely react with 75.00. ml of a 1.3 M KOH solution?

14. What is the molarity of H⁺ from question 13?

Define the following terms.

15. Solute

16. Solvent

17. Saturated solution

18. Unsaturated solution

19. Supersaturated solution

20. Molarity

21. Solubility

27. Molarity

28. Molality

29. Label and name the following as acids or bases.

a. H₃PO₄ e. KOH

b. NH₄ f. H₂SO₄

c. HNO₃ g. H₂CO₃

d. NaOH h. HF

30. For the following reactions indicate the acid, base conjugate acid and conjugate base.

A. H₃PO₄ + H₂O --> H₃O⁺ + H₂PO₄^-

B. NH₃ + H₂O --> OH^- + NH₄⁺

31. Explain the difference between a strong acid and a weak acid.

32. What are the products of neutralization reactions?

33. Write net ionic equations for the following reactions.

A. H₂CO₃ + Fe --> FeCO₃ + H₂

B. CaS + Fe(ClO₃)₂ --> FeS + Ca(ClO₃)₂

34. What is a polyprotic acid? What is a monoprotic acid? Give two examples of each.

35. The first hydrogen ion in a particular polyprotic acid is considered strong. What can you say about the remaining hydrogen ions?

36. Solve the following problems.

A. [H₃O⁺] = 1.43 x 10^-5 M

pH =

pOH =

[OH^-] =

B. [H₃O⁺] = 5.43 x 10^-10 M

pH =

pOH =

[OH^-] =

C. pOH = 12.2

pH =

[H₃O⁺] =

[OH^-] =

D. pOH = 1.53

pH =

[H₃O⁺] =

[OH^-] =

E. [OH^-] = 1.42 x 10^-5

pH =

[H₃O⁺] =

pOH =

F. [OH^-] = 3.14 x 10^-12

pH =

[H₃O⁺] =

pOH =

G. pH = 2.75

pOH =

[H₃O⁺] =

[OH^-] =

Gas laws

37. A 5.0 L tank of oxygen gas is at a pressure of 1.5 atm. What volume of oxygen will be available if the oxygen is used at standard atmospheric pressure?

38. A 100 L volume of gas is at a pressure of 460 mm of Hg and has a temperature of 56 C. What is the new temperature, in degrees Celsius, if the volume of the gas is unchanged and the new pressure is .785 atm?

39. How many moles of hydrogen (H₂) fill a weather balloon whose volume is 175 L at a pressure of 0.50 atm with a temperature of –25.0°C?

40. What is the resulting volume of 0.825 L of gas when it is cooled from 32.0°C to 20.0°C and subjected to a pressure change from 1.35 atm to 1.00 atm?

41. How many kilograms of oxygen must be placed in a container with a volume of 2.50 m³ to produce a pressure of 458 kPa at standard temperature?

42. Ammonia gas (NH₃) combines with oxygen gas to form nitrogen gas and water. If 3.5 L of ammonia are consumed in the reaction, how many cm³ of nitrogen are produced?

43. What mass of water is produced if 25.00 ml of butane (C₄H₁₀) reacts with oxygen at STP?