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|Arabia Mountain High School |Sample Final Examination |
|Chemistry |Answer using a #2 pencil |
|Version A |Bubble the correct answer on the scantron. |
|Write this version on your Scantron! | |
1. Liquid propane boils at -42 o C. What is this temperature according to the Kelvin scale?
A. 231 K
B. 255 K
C. 273 K
D. 315 K
2. The unbalanced equation for the reaction between iron (III) chloride and ammonium hydroxide is given below. According to the correctly balanced equation, how many grams of ammonium chloride (NH4Cl) would be produced when 2.0 moles of ammonium hydroxide (NH4OH) reacts completely.
1FeCl3 + 3NH4OH (1Fe(OH)3 + 3NH4Cl
A. 53.5 g
B. 26.8 g
C. 107 g
D. 80.3 g
3. According to the law of conservation of mass, when sodium, hydrogen and oxygen react to form a product, the mass of the products compared to the mass of the reactants will be _____.
A. greater
B. equal
C. less
D. none of the above
4. Balance the equation below and determine how many moles of CaCl2 would be produced from 12 moles of SbCl3.
3CaSi2 + 2SbCl3 ( 6Si + 2Sb + 3CaCl2
A. 1
B. 3
C. 6
D. 18
5. Based on the following balanced reaction, if you have 8 moles of AlCl3 and 9 moles of MgSO4, which is your limiting reactant?
2AlCl3 + 3MgSO4 ( Al2(SO4)3 + 3MgCl2
A. AlCl3
B. MgSO4
C. Al2(SO4)3
D. MgCl2
6. For the reaction listed below: If 3 moles of phosphorus react with 10 moles of oxygen, the theoretical yield of phosphorus (V) oxide will be _____.
P4 (s) + 5O2 (g) ( P4O10 (s)
A. l mol
B. 2 mol
C. 3 mol
D. 10 mol
7. How many moles are in 265 grams of Na2CO3?
A. 0.15
B. 2.5
C. 3.2
D. 1.5 x 1024
8. If 40.0 g of HCl and 15.0 g of Al(OH)3 react according to the following balanced equation, how many grams of water will be produced?
3HCl (aq) + Al(OH)3 (aq) ( AlCl3 (aq) + 3H2O (l)
A. 28.5 g
B. 10.4 g
C. 21.1 g
D. 19.8 g
9. In the chemical equation CaO (s) + CO2 (g) ( CaCO3 (s) , 1.5 mol of CaCO3 will form from _____.
A. 3 mol of CaO and 3 mol of CO2
B. 1.5 mol of CaO and 1.5 mol of CO2
C. 1 mol of CaO and 2 mol of CO2
D. 3 mol of CaO and 6 mol of CO2
10. Reaction stoichiometry involves the _____.
A. amounts of reactants and products in a reaction
B. mass of a single reactant or product
C. temperature change during a chemical reaction
D. types of bonds in a chemical reaction
11. Rust is formed when iron combines with the oxygen in the air according to the reaction given below. How many grams of rust are formed when 16.7 g of iron react completely with oxygen?
4Fe (s) + 3O2 (g) ( 2Fe2O3 (s)
A. 12.0g
B. 23.9g
C. 47.8g
D. 95.6g
12. The correct mathematical expression for the relationship between percent yield, actual yield, and theoretical yield is ________.
A. [pic]
B. [pic]
C. [pic]
D. [pic]
13. The molar mass of aluminum oxide is _____ g/mol.
A. 43
B. 70
C. 75
D. 102
14. The substance that restricts the amount of product formed in a chemical reaction is known as the _____.
A. excess reactant
B. limiting product
C. limiting reactant
D. excess product
Use the following equation to answer questions 24-26.
C6H12O6 + O2 ( CO2 + H2O + energy
15. This equation represents the process known as _____.
A. photosynthesis
B. respiration
C. dehydration
D. polymerization
16. This reaction is _____.
A. endothermic
B. exothermic
C. neither
17. The coefficients needed to balance this equation are as follows _____.
A. 2, 1, 3, 1
B. 1, 6, 6, 4
C. 2, 12, 12, 10
D. 1, 6, 6, 6
18. A chemical reaction that uses energy is _____.
A. endothermic
B. thermonuclear
C. combustion
D. exothermic
19. A crystal of copper sulfate is added to a copper sulfate solution. After 15 minutes the crystal is observed in the bottom of the solution unchanged. On the basis of this observation, the solution is best described as _________________.
A. supersaturated
B. dilute
C. saturated
D. unsaturated
20. When chemicals are mixed in a test tube, the test tube becomes hotter. What kind of reaction has occurred?
A. exogenic
B. exothermic
C. endogenic
D. endothermic
21. In the combustion of propane, C3H8, the products are ______________.
A hydrogen
B. carbon dioxide and water
C. oxygen and water
D. oxygen
22. Give the reaction type for the following equation. 2C2H2 + 5O2 -----> 4CO2 + 2H2O
A. combustion
B. decomposition
C. single replacement or displacement
D. double replacement or displacement
23. For an exothermic reaction, the products __________.
A are at the same energy level as the reactants
B. have no energy
C. are at a lower energy level than the reactants
D. are at a higher energy level than the reactants
24. As the temperature of a substance increases, the average kinetic energy of its particles _____________.
A increases
B. decreases
C. remains constant
D. increases, then decreases
25. What are the standard conditions of temperature and pressure?
A. 0 degrees C and 1 atm pressure
B. -273 degrees C and 1 atm pressure
C. 273 degrees C and 760 mmHg pressure
D. 0 K and 1 atm pressure
26. What volume will one mole of a gas occupy under STP (Standard Temperature and Pressure)?
A. L
B. 22.4 L
C. 273 L
D. 293 L
27. No molecular motion occurs ____________.
A. at night
B. in the atmosphere
C. at absolute zero
D. at the freezing point
28. A solution of _______ would not conduct an electric current.
A NaCl
B. HCl
C. C6H12O6
D. NH4Cl
29. If a sample of hydrogen gas and a sample of chlorine gas both occupy 67.2 L at STP, then __________.
A. they both contain a mole of particles
B. they both contain 3 moles of particles
C. the chlorine gas contains more particles
D. the hydrogen gas contains more particles
30. If a sample of Neon gas is allowed to expand to double its original volume at constant pressure, the temperature of the gas would __________________.
A. remain the same
B. increase
C. decrease
D. double
31. All of the following are units of pressure except
A. mmHg
B. atm
C. kPa
D. K
32. As the temperature increases, the motion of particles in a liquid ______________.
A. increases
B. decreases
C. remains the same
D. decreases then increases after one (1) hour of heating
33. What do the letters STP stand for?
A. stop try proceed
B. standard time process
C. standard temperature and pressure
D. stable temperature and pressure
34. A mixture that was cloudy, showed no settling, and had a positive Tyndall effect would be classified as a ________________.
A. colloid
B. suspension
C. solution
D. solvent
35. A solution in which water is the solvent is called a(n) ____________ solution.
A. immisicible
B. aqueous
C. astroid
D. nonpolar
36. A __________ is a substance that can dissolve another substance.
A. solute
B. solvent
C. saturation
D. solution
37. A ______________ solution holds more than the maximum amount of solute at a given temperature.
A. saturated
B. dilute
C. supersaturated
D. unsaturated
38. If you increase the temperature of a reaction, the rate of the reaction will often _______________.
A. increase
B. decrease
C. cause no change in
39. Identify the solvent in a salt water solution.
A. Salt
B. Water
C. Neither
D. Both
40. Which of the following would increase the rate of the reaction?
A. heating the test tubes in a water bath
B. cooling the test tubes
C. decreasing the concentration of the reactants
41. A common household acid is ___________.
A. ammonia
B. vinegar
C. soap
D. water
42. A pH of ___ is neutral.
A. 1
B. 7
C. 10
D. 14
43. A solution that changes color based on pH is called a(n) ____.
A. acid
B. base
C. hydroxide
D. indicator
44. A solution that contains hydronium ions can best be defined as a(n) ____________________.
A. neutral
B. acid
C. base
D. salt
45. A solution that resists pH change is a(n) _____________.
A. acid
B. base
C. reactant
D. buffer
46. Drano, a drain cleaner, will turn red litmus paper blue, it turns bright pink with phenolphthalein, and feels slippery if it gets on your skin. Drano has a pH _____________.
A. below 7
B. above 7
C. of 7
D. that cannot be determined without testing
47. Fruits such as lemons contain __________ acid.
A. lactic
B. acetic
C. citric
D. nitric
48. Predict the products of the following neutralization reaction. HCl + NaOH ----------> _______ + _______
A. Na2O; H2Cl
B. HNa; ClOH
C. NaCl; H2O
D. HNaO; Cl2
49. ______ is an example of a polyprotic acid.
A. HCl
B. HNO3
C. H2SO4
D. NaOH
50. A solution with a pH of 6.5 would be classified as a(an) _________.
A. Neutral solution
B. Acid
C. Base
51. A substance that contains hydrogen and releases H+ in solution is known as a(n) ______________.
A. acid
B. base
C. neutral substance
D. alkaline substance
52. An acid spill can be neutralized by adding ________.
A. vinegar
B. phenolphthalein
C. salt
D. baking soda
53. Ammonia can be considered a base because it can accept _______.
A. electrons
B. protons
C. hydroxide ions
D. neutrons
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