Chapter 6:
Chemical Reactions and Equations
Practice Test
1.
A solid that forms from a solution during a chemical reaction is called a ______________.
a.
precipitate
b.
reactant
c.
formate
d.
substrate
Hint
2.
A ____________ reaction is one in which a compound breaks down into two or more simpler substances.
a.
photosynthesis
b.
decomposition
c.
synthesis
d.
replacement
Hint
3.
________________ indicate a state of equilibrium in a chemical equation.
a.
Double reaction arrows
b.
A minus sign
c.
A plus sign
d.
An equal sign
Hint
4.
A number placed before a formula to indicate how many units of the substance are involved in a chemical reaction is called a ____________.
a.
coefficient
b.
substrate
c.
subscript
d.
superscript
Hint
5.
A description of a chemical reaction that includes the names of all reactants and products, but not the formulas, is called a ___________________.
a.
word equation
b.
skeleton equation
c.
chemical equation
d.
balanced equation
Hint
6.
The substances to the left of the reaction arrow are called _______________.
a.
reactants
b.
precipitates
c.
products
d.
gases
Hint
7.
What is the missing product in this balanced equation describing the decomposition of water? 2H
2
O(l) + energy
O
2
(g) +
a.
energy
b.
H
2
O(g)
c.
2H
2
(g)
d.
H
2
(g)
Hint
8.
Changes in energy, color, and odor are indications that a __________ has taken place.
a. separation reaction
b. displacement reaction
c. chemical reaction
d. precipitation reaction
Hint
9.
A ____________ reaction is one in which one element takes the place of another in a compound.
a.
double displacement
b.
synthesis
c.
decomposition
d.
single displacement
Hint
10.
The substances to the right of the reaction arrow are called _______________.
a.
gases
b.
products
c.
reactants
d.
precipitates
Hint
11.
This type of chemical reaction has energy written as a product.
a.
energy-absorbing
b.
light-absorbing
c.
endothermic
d.
exothermic
Hint
12.
Adding energy to an equilibrium system that is exothermic to the right causes the system to ______________.
a.
shift to the left
b.
slow down
c.
shift to the right
d.
remain unchanged
Hint
13.
What is the coefficient for NaOH in the equation that describes its reaction with CO
2
to produce Na
2
CO
3
and H
2
O?
a.
1
b.
2
c.
3
d.
4
Hint
14.
What type of reaction is represented by the equation Pb(NO
3
)
2
+ K
2
CrO
4
PbCrO
4
+ 2KNO
3
?
a.
double displacement
b.
single displacement
c.
decomposition
d.
synthesis
Hint
15.
A reaction between magnesium chloride and silver nitrate yields magnesium nitrate and silver chloride. What is the coefficient for magnesium nitrate in the balanced equation for the reaction?
a.
2
b.
3
c.
4
d.
1
Hint
16.
The positive and negative portions of two ionic compounds are interchanged in this type of reaction.
a.
synthesis
b.
single displacement
c.
decomposition
d.
double displacement
Hint
17.
What type of reaction is represented by the equation 2Fe + 3Cl
2
2FeCl
3
?
a.
synthesis
b.
combustion
c.
decomposition
d.
single displacement
Hint
18.
Changes in an equilibrium system can be described according to _____________ principle.
a.
Boyle's
b.
Le Chatelier's
c.
Dalton's
d.
Rutherford's
Hint
19.
What type of reaction is represented by the equation CH
4
+ 2O
2
CO
2
+ 2H
2
O?
a.
combustion
b.
double displacement
c.
synthesis
d.
decomposition
Hint
20.
Reactions that can occur in either direction are said to be ____________.
a.
forward
b.
backward
c.
limited
d.
reversible
Hint
