Matter Test

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Chemistry Test

Unit Two

Chapter 3

 

Choose the best answer to each of the following questions.

  1. Which of the following describes the carbon dioxide gas dissolved in a carbonated beverage?
  1. solute
  2. solvent
  3. precipitate
  4. solution

 

2. A chemical change must produce which of the following?
  1. a new substance
  2. a gas
  3. a solution
  4. a mixture

 

3. Which of the following is a chemical property of the element magnesium?
  1. it melts at 650 oC
  2. it has density of 1.738 g/ml
  3. it is easily bent
  4. it easily dissolves in acid

 

4. Refer to the graph below. What is the solubility of KBr at 30 oC?

    1. 75 g/100 g of water
    2. 65 g/100 g of water
    3. 70 g/100 g of water
    4. 30 g/100 g of water

 

5. Which of the following is classified as a homogeneous mixture?

  1. ice
  2. sugar dissolved in water
  3. sand in water
  4. iron fillings in water

 

6. The energy required to raise the temperature of one gram of a substance by one degree celsius is called ___________ for that substance.
  1. the melting point
  2. the specific heat capacity
  3. the joule
  4. the density

 

7. A reaction in which heat is release is said to be ___________
  1. exothermic
  2. endothermic
  3. isothermic
  4. nonspontaneous

 

8. Which of the following is a characteristic of pure substances?
  1. they are solutions
  2. they are mixtures
  3. they are composed of one substance
  4. they have a constant boiling point

 

9. Which of the following is an example of a pure substance?
  1. salt water
  2. copper
  3. stained glass
  1. chocolate chip ice cream

 

10. Which of the following is an incorrect statement about compounds?
  1. compounds are composed of elements in definite proportions
  2. compounds can be liquids, solids or gases
  3. compounds can be ionic or covalent
  4. compounds can easily be broken apart

 

11. The correct chemical formula for a compound containing two atoms of hydrogen and two atoms of oxygen per molecule is
  1. H2O
  2. 2H2O
  3. H2O2
  4. 2OH2

 

12. How much heat energy would be lost by the cooling of a gold ingot with a mass of 1.490 grams from 591.0 oC to 35.00 oC? The specific heat capacity for gold is 0.12905 J/g oC?

    1. 107 J
    2. 106.9 J
    3. 106.91
    4. 106.910

For questions 13, 14 and 15, refer to the drawings below

13. Which of the figures represents a heterogeneous mixture that is a liquid?
  1. a
  2. b
  3. c
  4. d
  5. e

 

14. Which of the figures represents a pure solid?
  1. a
  2. b
  3. c
  4. d
  5. e

 

15. Which of the figures represents a heterogeneous mixture that is a solid?
  1. a
  2. c
  3. e
  4. f
  5. g

 

Free Response

You must show all work to receive full credit
  1. Use the concepts of kinetic energy and mean free paths to describe what happens when a solid is heated until it melts.

 

  2.  Suppose that you held in your hand a beaker that contained an       
       endothermic reaction. What would you feel?

  3. Classify each of the following as physical or chemical changes. For 
      each chemical change, cite the observable evidence that indicates 
      that this is the kind of change occurring.

    1. melting ice
    2. fizzing of an antacid tablet in water
    3. rusting of iron
    4. dissolving sugar in iced tea
    5. exploding firecrackers

 

  1. 4. How much heat energy is required to raise the temperature of 500.0 g of water from 30.00 oC to 38.00 oC? The specific heat capacity for water is 4.18 J/g oC

 

  1. An unknown metal is brought into the lab. You decide to perform an experiment to determine the specific heat capacity of the metal. You collect the following data:

Mass of metal = 1.070 g

Initial temperature of metal = 97.7 oC

Volume of water in calorimeter = 25.0 ml

Initial temperature of water in calorimeter = 22.3 oC

Final temperature of water in calorimeter = 27.9 oC

The specific heat capacity for water = 4.18 J/g oC.

What is the specific heat capacity for the metal?