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Chapter 5:  Chemistry in Action

 1. 
Every chemical reaction involves a change in
A.
mass.
B.
energy.
C.
concentration.
D.
state.
 

 2. 
A reaction that absorbs energy in the form of heat is described as
A.
endothermic.
B.
exothermic.
C.
combustion.
D.
unbalanced.
 

 3. 
Which process changes matter into one or more new substances with new properties?
A.
physical change
B.
chemical change
C.
conservation
D.
freezing
 

 4. 
What happens when chemical bonds break and new bonds form?
A.
a physical change
B.
a chemical reaction
C.
matter is destroyed
D.
surface area increases
 

 5. 
A solid that forms from solution during a chemical reaction is called a
A.
reactant.
B.
bond.
C.
chemical.
D.
precipitate.
 

 6. 
A shorter, easier way to show chemical reactions, using symbols instead of words, is called a
A.
chemical equation.
B.
chemical formula.
C.
symbol.
D.
subscript.
 

 7. 
The substances listed on the left side of a chemical equation are the
A.
products.
B.
coefficients.
C.
precipitates.
D.
reactants.
 

 8. 
Sulfur dioxide, oxygen, and water combine to produce sulfuric acid (2 SO2 + O2 + 2 H2O -> 2 H2SO4). This chemical reaction is
A.
an example of combustion.
B.
a synthesis reaction.
C.
a replacement reaction.
D.
a decomposition reaction.
 

 9. 
In chemical reactions, what does the principle of conservation of mass mean?
A.
Matter is not created or destroyed.
B.
The total mass of the reactants is greater than the total mass of the products.
C.
The total mass of the reactants is less than the total mass of the products.
D.
Matter is not changed.
 

 10. 
Which of the following is a balanced chemical equation?
A.
H2O2 -> H2O + O2
B.
2 Fe2O3 + 3 C -> 4 Fe + 3 CO2
C.
SO2 + O2 + 2 H2O -> 4 H2SO4
D.
2 Mg + HCl -> MgCl2 + H2
 

 11. 
In an equation, numbers often appear in front of a chemical formula. These numbers tell you the
A.
number of atoms in each molecule in the reaction.
B.
number of elements in the reaction.
C.
number of molecules or atoms of each substance in the reaction.
D.
number of molecules in each atom in the reaction.
 

 12. 
When two or more substances combine to make a more complex compound, the process is called a
A.
decomposition reaction.
B.
replacement reaction.
C.
precipitate reaction.
D.
synthesis reaction.
 

 13. 
A bottle of hydrogen peroxide that eventually turns into a bottle of water and oxygen gas is an example of a
A.
synthesis reaction.
B.
decomposition reaction.
C.
replacement reaction.
D.
precipitate reaction.
 

 14. 
The chemical reaction between copper oxide and carbon that produces copper and carbon dioxide (CuO + C -> Cu + CO2) is an example of
A.
synthesis.
B.
decomposition.
C.
precipitation.
D.
replacement.
 

 15. 
The minimum amount of energy that has to be added to start a reaction is the
A.
exothermic energy.
B.
endothermic energy.
C.
activation energy.
D.
chemical energy.
 

 16. 
Chemicals that act as biological catalysts by speeding up reactions in living things are
A.
inhibitors.
B.
enzymes.
C.
fuels.
D.
reactants.
 

 17. 
A material used to decrease the rate of a chemical reaction is a(n)
A.
inhibitor.
B.
catalyst.
C.
enzyme.
D.
fuel.
 

 18. 
Which of the following would increase the rate of a reaction ?(choose all correct answers)
 A.
Grinding a solid into a powder
 B.
Cooling the reactants
 C.
Heating the reactants
 D.
Adding an inhibitor
 E.
Adding a catalyst
 F.
Decreasing the concentration of reactants
 
 
nar001-1.jpg
 

 19. 
The diagram above shows the energy change is which type of reaction?
A.
Endothermic
B.
Exothermic
 
 
nar002-1.jpg
 

 20. 
The diagram above shows the energy change in which type or reaction?
A.
Endothermic
B.
Exothermic
 

 21. 
Only exothermic reactions require activation energy.
 

 22. 
A catalyst participates in a chemical reaction and is changed into a new product by the reaction.
 

 23. 
“Matter is neither created nor destroyed during a chemical reaction” is best described by what law?
A.
Boyle’s
B.
Charles’
C.
Conservation of Mass
D.
Contribution of Density
 



 
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