1. On heating, Cl₂O₇ decomposes to form Cl₂ and O₂. What is the ratio of chlorine to oxygen molecules in the product?

(A) 2 to 7
(B) 2 to 14
(C) 3 to 7
(D) 4 to 7

2. One mole of an element contains 4.82 x 10²⁴ electrons. What is the atomic number of the element?

(A) 2
(B) 4
(C) 6
(D) 8

3. Which physical property would be most useful for determining whether two samples of metal are the same metal?

(A) mass
(B) volume
(C) color
(D) density

4. Which technique could be used to separate a homogeneous mixture?

Techniques:
I. chromatography
II. distillation
III. filtration

(A) I only
(B) III only
(C) I and II only
(D) I, II, III

5. The addition of which solution would provide the best way to distinguish between AgNO_3(aq) and Zn(NO₃)_2(aq)?

(A) H₂O
(B) HNO₃
(C) NH₃
(D) HCl

6. Equal masses of O₂ and N₂ are reacted according to this equation:

O₂ + N₂ → 2 NO

Which statement is true?

(A) O₂ is the limiting reagent and N₂ is present in excess
(B) N₂ is the limiting reagent and O₂ is present in excess
(C) all of the O₂ and N₂ react and neither is in excess
(D) Nothing can be said about the limiting reagent

7. When a 0.817 g sample of a copper oxide is heated with excess hydrogen gas, 0.187 g of water is formed. What is the apparent formula of the copper oxide?  [Cu = 63.5, O = 16]

(A) CuO
(B) Cu₂O
(C) Cu₂O₃
(D) CuO₂

8. A lab manual directs a student to measure a piece of ribbon 5.00 cm long and calculate its mass from the mass of 100.00 cm of the ribbon (0.985 g). Why is this approach superior to simply cutting a 5.00 cm piece of ribbon and determining its mass on an electronic milligram balance?

(A) Magnesium ribbon can corrode the balance pan as it is being weighed
(B) Such a small piece of ribbon will not give a readout on a milligram balance
(C) The length can be measured more rapidly than the mass
(D) Measuring its length gives a more precise mass

9. A particular chlorofluorocarbon (CFC) contains 9.93% C, 31.43% F, and 58.64% Cl by mass. Its molar mass is 120.9 g/mol. How many F atoms are in one molecule?          [ C = 12, Cl = 35.5, F = 19]

(A) 1
(B) 2
(C) 3
(D) 4

10. Which is the strongest acid?

(A) HF
(B) HNO₂
(C) H₂SO₄
(D) H₃PO₄

11. Which piece of glassware should be used to measure 8.70 mL of a solution?

(A) 20-mL graduated cylinder
(B) 25-mL volumetric flask
(C) 50-mL buret
(D) 100-mL beaker

12. The density of an insoluble object is determined by weighing it on a balance, then submerging it in a graduated cylinder to find its volume. Based on the data collected, to how many significant figures should the density be reported?

(A) 1
(B) 2
(C) 3
(D) 4

13. The formula of sodium tungstate is Na₂WO₄ and that of lead phosphate is Pb₃(PO₄)₂. What is the formula for lead tungstate?

(A) PbWO₄
(B) Pb₂(WO₄)₃
(C) Pb₃(WO₄)₂
(D) Pb₃(WO₄)₄

14. When 500.0 mL of 1.0 M LaCl₃ and 3.0 M NaCl are mixed, what is the molarity of the chloride ion?

(A) 4.0 M
(B) 3.0 M
(C) 2.0 M
(D) 1.5 M

15. An aqueous solution is 0.1 M in each of these ions.

1. Cu²⁺
2. Hg²⁺
3. Pb²⁺

Which ion(s) will precipitate if 0.1 M HCI is added?

(A) 2 only
(B) 3 only
(C) 2 and 3 only
(D) 1,2, and 3

16. What is the coefficient for oxygen when this equation is balanced?

Sb₂S₃(s) + O₂(g) → Sb₂O₃(s) + SO₂(g)

(A) 9
(B) 7
(C) 5
(D) 4

17. Flourine reacts with uranium hexafluoride (UF₆) as represented by this equation.

U(s) + 3F₂(g) → UF₆(g)

How many flourine molecules are required to produce 2.0 mg of uranium hexafluoride (UF₆) from an excess of uranium?  [The molar mass of UF₆ is 352.0 g/mol]

(A) 3.4 x 10¹⁸
(B) 1.0 x 10¹⁹
(C) 2.0 x 10¹⁹
(D) 3.4 x 10²¹

18. Calculate the percent by mass of hydrogen in diethylamine ((C₂H₅)₂NH).    [ C =12, N = 14, H = 1]

(A) 11.3%
(B) 13.7%
(C) 15.2%
(D) 23.6%

19. 2.0 x 10^-3 mol of a chlorine containing compound, when placed in water, reacted completely with 80.0 cm³ of 0.05 M AgNO₃. The compound could be:

(A) NaCl
(B) MgCl₂
(C) AlCl₃
(D) TiCl₄

20. When these species (SO₂, PbS and Na₂S₂O₃) are listed in order of increasing oxidation number of the sulfur atoms, the correct order is

(A) PbS, Na₂S₂O₃, SO₂
(B) PbS, SO₂, Na₂S₂O₃
(C) Na₂S₂O₃, PbS, SO₂
(D) SO₂, Na₂S₂O₃, PbS

21. How many moles of ozone (O₃) could be formed from 48.0 g of oxygen gas?

(A) 1.00 mol
(B) 1.30 mol
(C) 1.50 mol
(D) 2.00 mol

22. Which formula represents a peroxide?

(A) Li₂O
(B) SiO₂
(C) Na₂SiO₃
(D) BaO₂

23. Chlorine reacts with fluorine above 200 °C to form chlorine trifluoride (ClF₃) as shown by this equation:

Cl₂(g) + 3F₂(g) → 2ClF₃(g)

If equal numbers of moles of chlorine and fluorine are combined, the maximum number of moles of ClF₃ that could be formed will be equal to:

(A) the number of moles of Cl₂.
(B) the number of moles of F₂.
(C) twice the number of moles of Cl₂.
(D) two-thirds the number of moles of F₂.

24. Each of three samples was weighed on a different balance. The masses of the three are 1.028 kg, 82.9 g, and 45.1 mg. The sum of the three masses should be reported as:

(A) 1110.9451 g
(B) 1111 g
(C) 110 g
(D) 1.11 x 10³ g

25. Antimony reacts with chlorine according to this equation:

2 Sb + 3 Cl₂ → 2 SbCl₃

How many grams of SbCl₃can be prepared if 0.0120 mol of antimony are reacted with 0.0200 mol of chlorine? [The molar mass of SbCl3 equals 228.2 g/mol]

(A) 1.52 g
(B) 1.83 g
(C) 2.74 g
(D) 4.56 g

26. The net ionic equation for the precipitation reaction that occurs when aqueous solutions of AgNO₃ and K₂CrO₄ are mixed is:

(A) K⁺ + NO₃¯ → KNO₃(s)
(B) Ag⁺ + CrO₄¯ → AgCrO₄(s)
(C) K₂⁺ + NO₃¯ → K₂NO₃(s)
(D) 2Ag⁺ + CrO₄²¯ → Ag₂CrO₄(s)

27. A car traveling at 10 miles per hour emits about 0.15 kg of carbon monoxide (CO) gas per mile. How many moles of CO are emitted per mile under theses conditions?    [C = 12, O = 16]

(A) 5.4 x 10^-1
(B) 5.4
(C) 9.4
(D) 12.5

28. The formula of the compound ammonium carbonate is:

(A) NH₄CO₃
(B) NH₄CO₄
(C) NH₄HCO₃
(D) (NH₄)₂CO₃

29. What is the number of molecules in 1.00 mL of a gas at STP?

(A) 2.69 x 10²²
(B) 6.02 x 10²⁰
(C) 2.69 x 10¹⁹
(D) 22.4 x 10¹⁹

30. In the reaction

6 KI + 2 KMnO₄ + 4 H₂O → 3 I₂ + 2 MnO₂ + 8 KOH

Which atom undergoes oxidation?

(A) K
(B) Mn
(C) O
(D) I

31. Which quantity of nickel has the largest mass?    [Ni = 58.7]

(A) one mole
(B) 6.02 x 10²³ atoms
(C) 5.87 grams
(D) 2.4 moles

32. Which ion, in solution, can be oxidized by appropriate chemical means but also can be reduced by a different chemical reaction?

(A) Fe²⁺
(B) F¯
(C) CO₃²¯
(D) NO₃¯

33. If the smallest whole-number coefficients are used to balance the oxidation-reduction reaction

Cr₂O₃ + Na₂CO₃ + KNO₃ → Na₂CrO₄ + CO₂+ KNO₂

The sum of the coefficients in the balanced equation is:

(A) 13
(B) 14
(C) 17
(D) 19

34. The term that is related to the reproducibility or repeatability of a measurement is:

(A) accuracy
(B) systematic
(C) precision
(D) qualitative

35. If 18.5 moles of the liquid compound C₂Cl₄ are required for a particular chemical reaction, what volume should be taken? [The density of C₂Cl₄ is 1.63 g/ml, its molar mass is 166 g/mol]

(A) 11.3 mL
(B) 30.2 mL
(C) 1.88 L
(D) 5.01 L

36. 40.00 mL of 0.0900 M NaOH is diluted to 100.00 mL with distilled water and 30.00 mL of 0.1000 M HCl are added. The  resulting solution is:

(A) acidic
(B) neutral 
(C) alkaline
(D) amphoteric