1. End-of-Semester Review
Unit 1: Skills and Processes of Chemistry

2. What is the purpose of the...
Fume hood
Broken glass bin
Chemical waste container

3. What does WHMIS stand for?

4. What does each symbol mean?

5. Convert 10.0 km/h into m/s.
Convert 0.51 m3 into mL (or cm3).
Find the volume in L of a 20.0 kg piece of zinc, given that the density of zinc is 5.01 g/mL.
Convert 2.67 g/mL into kg/L.
Convert the density of neon gas from x10-4 mg/mL into kg/L.
Convert 4.3 dm3 into cm3.

6. What is 60 + 83.2, using significant figures?

7. What is 610 ÷ 9.1, using significant figures?
What is 4.59 X 3.201, using significant figures?
What is X 19.5, using significant figures?
What is ÷ 67000, using significant figures?
What is X , using significant figures?

8. Name each piece of lab equipment:

9. End-of-Semester Review
Unit 2: The Nature of Matter

10. Name the Vocab Word Anything that has mass and occupies space.
Something with a unique and identifiable set of properties.

11. Name the Vocab Word
A property that can be found without creating a new substance.
The ability of a substance to undergo chemical reactions and change into new substances.

12. Fill-in-the-Blanks
___ of the particles in a solid are ______ into a given volume in a highly __________ and rigid manner that requires particles to be in direct _______ with each other.
A liquid is a substance that ________ to the _____ of its container and experiences ______ changes in volume when ______ or subjected to ________ (not ____________).
The particles in a gas are ______ separated and only contact each other during __________.

13. Types of Particles Ag Identify the NO3- atoms molecules Cl- H2O H
5 min
C12H22O11 Cu
CH3CH2OH
Na+

14. Give an Example Homogeneous substance Compound Heterogeneous substance
Pure substance

15. Describe the Separation Method
Distillation
Solvent Extraction
Recrystallization
Gravity Separation
Chromatography

16. A molecule can possess three types of kinetic energy. Name one.
What phases are present at each place in the graph below?

17. Write the Formula Calcium phosphide Tin(IV) sulphate Ammonium sulphate
Mercury(I) chloride
10 min

18. Name It!
Cu2O
FeS
U(SO4)2
Zn(CH3COO)2·2H2O

19. Name It!
CS2 SO
N2O4

20. End-of-Semester Review
Unit 3: Moles

21. How many moles of CH3OH are there in 0.250 g of CH3OH?

22. What is the percentage composition of H2SO4?
What is the percentage of water in CuSO4·5H2O?

23. How many moles of gas are contained in a balloon with a volume of 10
How many moles of gas are contained in a balloon with a volume of 10.0 L at STP?
How many moles of N atoms are there in 5.00x1017 N atoms?

24. A compound contains 58. 5% C, 7. 3% H, and 34. 1% N
A compound contains 58.5% C, 7.3% H, and 34.1% N. What is the empirical formula of the compound?

25. A particular variety of carbon atom has a mass of 2. 16x10-23 g/atom
A particular variety of carbon atom has a mass of 2.16x10-23 g/atom. What is the mass of a mole of this variety of carbon atom?

26. What mass of NaOH is contained in 3.50 L of 0.200 M NaOH?
What is the molarity of pure sulphuric acid, H2SO4, which has a density of g/mL?
What is the molarity of the CaCl2 in a solution made by dissolving and diluting g of CaCl2·6H2O to mL?

27. How many hydrogen atoms are there in 30 molecules of H3PO4?

28. What is the mass of 1.00x1012 atoms of Cl?
How many oxygen atoms are contained in 75.0 L of SO3(g) at STP?

29. The density of Hg(l) is 13. 6 g/mL
The density of Hg(l) is 13.6 g/mL. How many moles of Hg(l) are contained in 100 mL of Hg(l)?
Al2O3(s) has a density of 3.97 g/mL. How many atoms of Al are in 100 mL of Al2O3?

30. A 2. 50 L bulb contains 4. 91 g of a gas at STP
A 2.50 L bulb contains 4.91 g of a gas at STP. What is the molar mass of the gas?

31. What volume at STP is occupied by 5.34 g of neon gas?
What is the molar volume of mercury (density = 13.6 g/mL)?

32. A gas has the empirical formula POF3. If 0
A gas has the empirical formula POF3. If L of the gas at STP has a mass of 1.62 g, what is the molecular formula of the compound?

33. If 300. 0 mL of 0. 250 M NaCl is added to 500. 0 mL of 0
If mL of M NaCl is added to mL of M NaCl, what is the resulting [NaCl] in the solution?

34. A student mixes 100. 0 mL of water with 25
A student mixes mL of water with 25.0 mL of a NaCl solution having an unknown concentration. If the diluted solution has [NaCl] = M, what is the molarity of the original NaCl solution?

35. How many moles of N2 are there in 50.0 g of N2?
What is the mass of 1.36X10-3 mol of SO3?

36. What is the empirical formula of a compound containing 39.0% Si and 61.0% O?

37. The empirical formula of a compound is SiH3. If 0
The empirical formula of a compound is SiH3. If mol of a compound has a mass of 1.71 g, what is the compound’s molecular formula?

38. End-of-Semester Review
Unit 4: Chemical Reactions

39. Closed Systems Give an example of a system that is...
Closed with respect to light.
Open with respect to light but closed with respect to mass.
Closed with respect to sound.
Open with respect to mass and closed with respect to light.
Closed with respect to heat.
TPS - 5 min

40. What four quantities do not change during a chemical reaction in a closed system?

41. Balancing Equations
__Cr2(SO4)3 + __KI + __KIO3 + __H2O → __Cr(OH)3 + __K2SO4 + __I2 __MoCl3 + __O2 + __AgCl → __MoCl4 + __Ag2O
15 min

42. Writing Equations
Liquid water reacts with powdered sodium oxide to produce aqueous sodium hydroxide.
Aqueous hydrochloric acid reacts with calcium carbonate crystals, producing aqueous calcium chloride, gaseous carbon dioxide, and liquid water.
I do #1, then we do #2 and 3 – 25 min

43. Classify and Predict the Products:
N2(g) + F2(g)
ClN3(s)
2 HI(aq) + Co(s)
Pb(NO3)2(aq) + 2 NaBr(aq)
Al(OH)3(s) + H3PO4(aq)
C6H5OH + 7 O2

44. Enthalpy Sketch the potential energy graph for:
A) an exothermic reaction
B) an endothermic reaction
In which type do the surroundings feel colder?
Which type includes synthesis reactions?
Is ΔH positive or negative in each case?
Would energy be written on the left or right side of the equation in each case?

45. End-of-Semester Review
Unit 5: Stoichiometry

46. 4P + 5O2  P4O10
Suppose you have 7.35 g of P. How many grams of O2 do you need in order to completely react with the P you have?

47. C2H4 + 3 O2 → 2 CO2 + 2 H2O
How many grams of carbon dioxide are produced from the reaction of 20.0 grams of ethylene (C2H4) with excess oxygen?

48. H3PO4 + 3 NaOH → NaPO4 + 3 H2O
What volume of 0.10 M H3PO4 is needed to react with 27.0 mL of 0.48 M NaOH?

49. If 50.0 g of H2(g) react with 73.0 g of O2(g) according to the reaction
2 H2(g) + O2(g) → 2 H2O(l),
which reactant is present in excess and by how many grams?

50. If 23.8 g of FeCl2, 28.0 g of KNO3 and 60.0 g of HCl are mixed and allowed to react according to the reaction 3 FeCl2 + KNO3 + 4 HCl → FeCl3 + NO + 2 H2O + KCl
a) which chemical is the limiting reactant?
b) how many grams of each excess reactant are present in excess?

51. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l)
If a sample of propane (C3H8) is burned, what mass of water is produced if the reaction also produces 5.0 L of carbon dioxide at STP?

52. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l)
What volume of oxygen gas is consumed if 40.0 L of carbon dioxide gas at STP is produced?