The Nature of Chemical Reactions – Chapter 7 – Quiz Questions #1

  1. State the definition for REACTANT.

  2. State the definition for PRODUCT.

  3. State the definition for CHEMICAL ENERGY.

  4. State the definition for EXOTHERMIC REACTION.

  5. State the definition for ENDOTHERMIC REACTION.

  6. List three signs that could indicate that a chemical reaction is taking place.




  7. List four forms of energy that may be absorbed or released during a chemical reaction.





  8. In the following equation, what are the reactants and what are the products?

                      CH4   +    2O2     -------à   CO2    +      2H2O


Chemical Equations – Chapter 7 – Quiz Questions #2


2.What is a COEFFICIENT?

3.What is a SUBSCRIPT?

4.Balance the following chemical equations:

a)       H
2O        à        H2           +         O2
               water            (yields)      hydrogen         +                oxygen

b)       KOH             +       HCl              à            KCl           +     H2O
             potassium hydroxide  +  hydrochloric acid         (yields)         potassium chloride   +        water

c)       NaHCO3         à      H2O       +      CO2           +    Na2CO3
             sodium bicarbonate    (yields)      water           +        carbon dioxide      +      sodium carbonate
                 (baking soda)

d)     FeS        +    2HCl          à        H2S               +         FeCl2  
             iron sulfide   +   hydrochloric acid   (yields)      hydrogen sulfide       +            iron chloride

e)     Mg          +       O2        à           MgO
             magnesium    +           oxygen       (yields)         magnesium oxide

f)      K            +       H2O      à           KOH                 +      H2
             potassium       +           water          (yields)            potassium hydroxide    +        hydrogen

g)     CuCl2          +       Al        à            AlCl3             +     Cu
             copper chloride     +   aluminum        (yields)             aluminum chloride   +        copper

h)     CH4          +       O2       à          CO2             +     H2O
             methane             +      oxygen         (yields)            carbon dioxide        +        water

      i)     CO2          +       H2O        à         C6H12O6      +          O2
                   carbon dioxide     +           water            (yields)            sugar                       +                oxygen

       j)     Fe          +       O2        à        Fe2O3
                    iron                +           oxygen      (yields)       iron oxide

       k)     N2          +       H2        à        NH3            
                    nitrogen           +          hydrogen     (yields)      ammonia

       l)     Cu2O          +       C        à        Cu         +     CO2
                   copper oxide           +         carbon     (yields)        copper           +        carbon dioxide


Reaction Types – Chapter 7 – Quiz Questions #3

  1. Define the term SYNTHESIS REACTION and give an example.
        a) Definition:

        b) Example:

  2. Define the term DECOMPOSITION REACTION and give an example.

        a) Definition:

        b) Example:

  3. Define the term COMBUSTION REACTION and give an example. 

        a) Definition:

        b) Example:

  4. Define the term SINGLE-DISPLACEMENT REACTION and give an example.

        a) Definition:

        b) Example:

  5. Define the term ELECTROLYSIS.

  6. Define the term DOUBLE-DISPLACEMENT REACTION and give an example.

        a) Definition:

        b) Example:

  7. What is a FREE RADICAL?

  8. Define the term REDOX REACTION and give an example.

        a) Definition:

        b) Example:

Reaction Rates – Chapter 7 – Quiz Questions #4

pp. 238 - 247

  1. List four factors that affect the rate of a reaction.
    a)                            b)                      c)                              d)

  2. Define the term CATALYST.

  3. Define the term ENZYME.

  4. Define the term SUBSTRATE.

  5. Substances that slow reactions are called ____________________.

  6. When you open a soda bottle, what change occurs that allows the dissolved carbon dioxide in the soda to come out of solution?

  7. Define the term CHEMICAL EQUILIBRIUM.

  8. What is Le Chatelier’s principle?

  9. Compare a catalyst and an inhibitor.

  10. The Haber process uses Le Chatelier’s principle to produce more ammonia. What two things do they have to do to the reaction to get more ammonia as a product?

Summary – Chapter 7 – Quiz Questions #5
p. 251

1. Chemical reactions occur when substances undergo __________ changes to form new substances.

2. Chemical reactions involve changes in __________.

3. A chemical equation uses __________ to represent a chemical reaction.

4. A balanced equation tells you the _______ ______, or proportion of ________ and ________, in a chemical reaction.

5. List four types of chemical reactions.

6. Free-radical reactions and redox reactions can be understood as changes in the number of __________ that atoms have.

7. Anything that increases _________ between particles will increase the rate of a reaction.

8        . Process that go in both directions may result in ______________.