1. Chemistry
2004 Released Test

2. 10.0 mL graduated cyclinder
1. If a student needed to obtain 8.0 mL of a liquid for an experiment, the appropriate piece of laboratory equipment to use would be a —
50 mL beaker
1.0 mL pipet
50 mL flask
10.0 mL graduated cyclinder 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

3. 2. How many grams of sodium chloride are required to prepare 500
2. How many grams of sodium chloride are required to prepare mL of a M solution?
1.46 g
2.93 g
29.3 g
58.5 g 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

4. To produce a variety of results To include another variable
3. Which of the following best describes why an experiment should be repeated?
To organize the date
To produce a variety of results
To include another variable
To verify the observed results 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

5. 4. Which of these is the general formula for a double-replacement reaction?
A + B → AB
AB + XY → BA + YX
AB + XY → AY + XB
A + B + XY → AX + BY 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

6. 5 The correct formula of an ionic compound containing Al3+ and CO3 2- is —
AlCO3
Al(CO3)3
Al2(CO3)3
Al3(CO3)2 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

7. 6. Which of the following orbital diagrams is incorrect because it violates Hund’s rule?
Picture Choice 1
Picture Choice 2
Picture Choice 3
Picture Choice 4 B. C. D. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

8. 7. The graph shows the rate of a certain reaction as a function of temperature. According to the graph, in order to double the rate of the reaction at 20C, the temperature must be increased by approximately —
10°C
20°C
30°C
40°C 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

9. 8. Which of the following is the balanced chemical equation for the reaction shown above?
Al + H2SO4 → Al2(SO4)3 + H2
2Al + 3H2SO4 → Al2(SO4)3 3H2
2Al + 3H2SO4 → Al2(SO4)3 + H2
2Al + H2SO4 → Al2(SO4)3 + H2 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

10. Flammability Health Reactivity Contact
9. If a lab group were using hydrochloric acid to perform a substitution reaction, which precaution would not be a concern?
Flammability
Health
Reactivity
Contact 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

11. 10. How many grams of product Z will be formed if 12
10. How many grams of product Z will be formed if 12.0 g of W react with 10.0 g of X to form 8.0 g of product Y in the reaction shown?
8.0 g
10.0 g
12.0g
14.0 g 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

12. 11. The figure below shows a compound containing hydrogen (H) and an unknown element Z. To which group on the periodic table does element Z belong? 13 14 15 16 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

13. Precise but not accurate Accurate but not precise Accurate and precise
12. A student obtained these data after measuring the mass of an object three different times. If the true value of the object’s mass is g, these data are best described as —
First measurement: g
Second measurement: g
Third measurement: g
Precise but not accurate
Accurate but not precise
Accurate and precise
Neither accurate nor precise 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

14. 13. Which of the following is the name of the molecule PCl3?
Phosphorus trichloride
Phosphorus chloride
Potassium trichloride
Potassium chloride 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

15. 14. What is the main similarity among elements in group 2?
Atomic radius
Chemical properties
Mass number
Boiling point 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

16. 15. A team of chemistry students made the above measurements and density calculations of the same type of material. The accepted value (true value) of the density of the material is 5.72 g/cm3. Which trial has the least amount of absolute error? 1 2 3 4 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

17. 16. The gas with the largest volume at STP is -
10.0 g He
10.0 g Ne
10.0 g Ar
10.0 g Kr 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

18. 17. A neutral atom of aluminum -27 contains
13 protons and 27 electrons
14 protons and 13 neutrons
13 electrons, 13 protons, and 14 neutron
13 electrons, 14 protons, and 13 neutrons 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

19. 18. Which of the following could cause a gaseous substance to liquify?
An increase in pressure
An increase in volume
An increase in Temperature
A decrease in number of moles 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

20. 19. The appropriate model for a decompostion reaction is -
Picture Choice 1
Picture Choice 2
Picture Choice 3
Picture Choice 4 B. C. D. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

21. 20. According to Charles’ law, the volume of a fixed amount of gas is directly proportional to -
Isoelectric mixture
Vapor concentration
Barometric pressure
Kelvin temperature 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

22. 21. Which of the elements is a positive ion with a charge of one?3 4 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

23. 22. The energy required to melt a solid into a liquid is called -
Heat of vaporization
Heat of fusion
Cooling curve
Triple point 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

24. 23. Cations are formed when neutral atoms lose -
Electrons
Protons
Neutrons
positron 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

25. 24. What is represented by the pH of a solution?
Partial pressure of hydrogen ion in the solution
Electronegativity of dissociated hydrogen ions in the solution
Concentration of hydrogen ions in the solution
Temperature of hydrogen ions in the solution 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

26. 25. The formula for dinitrogen tetroxide is -
N2O4
N3O3
N2O2 NO 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

27. 26. Industrial deep-sea divers must breathe a mixture of helium and oxygen to prevent a disorienting condition known as nitrogen narcosis. If a diver’s tank is filled with a helium-oxygen mixture to a pressure of 170 atmospheres and the partial pressure of helium is 110 atmospheres, the partial pressure of the oxygen is —
60 atm
110 atm
140 atm
280 atm 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

28. 27. The figure shows an experimental setup used to separate the components of a colored ink sample. Which of the following describes this laboratory techniques?
Chromatography
Filtration
Decanting
Distillation 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

29. Atomic number Electronegativity Atomic radius Ionization energy
28. Which of the following properties decreases from left to right across a period?
Atomic number
Electronegativity
Atomic radius
Ionization energy 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

30. 29. A sample of nitrogen occupies 10. 0 liters at 25°C and 98. 7 kPa
29. A sample of nitrogen occupies 10.0 liters at 25°C and 98.7 kPa. What would be the volume at 20°C and kPa?
7.87 L
9.45 L
10.2 L
10.6 L 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

31. 30. What is the correct Lewis dot structure for arsenic?
Picture Choice 1
Picture Choice 2
Picture Choice 3
Picture Choice 4 B. C. D. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

32. 31. The empirical formula for a substance is CH2
31. The empirical formula for a substance is CH2. If the molecular mass of the substance is 56, the molecular formula is —
C2H4
C3H
C4H8
C5H10 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

33. 32. Water molecules in a sealed jar are in a state of dynamic equilibrium because water vapor molecules —
H2O(l) ↔ H2O(g)
Are condensing at the same rate that others are evaporating
Cease to form when the air in the jar becomes saturated
Are evaporating faster than they are condensing
Form only at high temperatures 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

34. 33. The diagram shows the structural formula of benzene
33. The diagram shows the structural formula of benzene. The empirical and the molecular formulas of benzene are, respectively —
CH, C2H2
CH, C3H3
C3H3, C6H6
CH, C6H6 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

35. 34. How many grams of nitrogen are present in 2 moles of HNO3?1 2 14 28 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

36. Filtration Extraction Distillation Crystallization
35. Which basic lab technique involves the separation of a mixture’s components through differences in particle size?
Filtration
Extraction
Distillation
Crystallization 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

37. 36. The graph shows the pressure of an ideal gas as a function of its volume. According to the graph, increasing the volume from 100 mL to 150 mL -
Decrease the pressure by 80 kPa
Decreases the pressure by 160 kPa
Increases the pressure by 80 kPa
Increases the pressure by 160 kPa 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

38. 37. When the above equation is balanced, the coefficient of the hydrochloric acid will be -2 3 4 6 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

39. Equilibrium shifts to produce more product
38. Which of the following occurs when a reaction in a solution is at equilibrium and more product is added to the solution?
Equilibrium shifts to produce more product
Equilibrium shifts to produce more reactant
No change will occur
The reaction will stop 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

40. 39. Each balloon was filled with an identical number of moles of gas
39. Each balloon was filled with an identical number of moles of gas. Which of the following best explains why balloon B is larger than balloon A?
The gas in balloon A is under less pressure.
The gas in balloon A is warmer.
The gas in balloon B is under more pressure.
The gas in balloon B is warmer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

41. 40. The atomic number corresponds to an atom’s number of-
Protons
Neutrons
Electrons
positrons 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

42. 41. Line D represents water
41. Line D represents water. If the atmospheric pressure in a flask is lowered to 70 kPa, water would boil at what temperature?
32°C
70°C
92°C
100°C 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

43. 42. How many moles of copper are equivalent to 3
42. How many moles of copper are equivalent to 3.44 x 1023 atoms of copper?
0.571 moles
1.75 moles
5.41 x 1021 moles
5.41 x 1022 moles 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

44. 43. Which element naturally occurs as a diatomic molecule?Zn C K H 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

45. 44. What is the molar mass of Al(No3)3?
57 g/mol
103 g/mol
165 g/mol
213 g/mol 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

46. 45. What shape does the molecule BF3 have?
Bent
Liniear
Tetrahedral
Trigonal planar 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

47. 46. What is the mass in grams of one mole of sulfur dioxide (SO)2?1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

48. 47. When the above equation is balanced, the coefficients in order are -
1, 1, 1, 1
2, 1, 1, 2
3, 1, 3, 2
3, 2, 2, 1 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

49. 48. Solid magnesium has a specific heat of 1. 01 J/gC
48. Solid magnesium has a specific heat of 1.01 J/gC. How much heat is given off by a 20.0 gram sample of magnesium when it cools from 70.0C to 50.0C?
202 J
404 J
808 J
1010 J 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

50. 49. Which graph represents the reaction shown above?
Picture Choice 1
Picture Choice 2
Picture Choice 3
Picture Choice 4 B. C. D. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32

51. 50. How should 0.000365 be expressed improper scientific notation?
3.65
3.65 x 10-4 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32