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WorksheetsCh 9, 15-18 Review
Total questions: 68
Worksheet time: 59mins
Name
Class
Date
1.
Chemical reactions are affected by collisions
a)
true
b)
false
2.
The minimum amt of energy needed for a reaction to take place is called ______ energy.
a)
activation
b)
potential
c)
kinetic
3.
Theory that states that atoms, ions and molecules must collide in order to react and in correct orientations
a)
collision
b)
big bang
c)
adhesion
4.
The ability to do work or produce heat
a)
energy
b)
metal
c)
a job
d)
combustion
5.
Adding or removing reactants or products in a reaction increases the number of collisions between molecules and stresses equilibrium.
a)
true
b)
false
6.
Exothermic reactions that have an increase in temperature shifts the reaction to the left toward the products.
a)
true
b)
false
7.
What does pH measure?
a)
how acidic a substance is
b)
how basic a substance is
c)
how acidic or basic substances are
d)
how many hydronium ions and acid produces
8.
Indicators change color in the presence of a(n) _______________.
a)
acid or base
b)
buffer
c)
water molecule
d)
ester
9.
A base has a ___________ taste.
a)
bland
b)
salty
c)
bitter
d)
sour
10.
A base has a _________________.
a)
sour taste
b)
positive ion
c)
slippery feel
d)
pH of 5
11.
A ___________ acid or base completely dissociates in solution easily.
a)
titrated
b)
neutral
c)
weak
d)
strong
12.
A ___________ acid or base partially dissociates in solution easily.
a)
titrated
b)
neutral
c)
weak
d)
strong
13.
Which of the following would be a weak base pH measurement?
a)
2
b)
8
c)
5
d)
11
14.
Acids have a __________ taste.
a)
bitter
b)
sour
c)
sweet
d)
bland
15.
What is the range of pH values in an acidic solution?
a)
below 7
b)
above 7
c)
15-239058204958
d)
pH = 7
16.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 13
17.
What is neutral on the pH scale?
a)
7
b)
14
c)
P shape
d)
D shape
18.
For the reaction...
SO2 + O2 ↔ SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.↔
SO2 + O2 ↔ SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.↔
a)
left
b)
right
c)
left and right
d)
neither left nor right
19.
For the reaction...
SO2 + O2 ↔ SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
SO2 + O2 ↔ SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
20.
For the reaction...
SO2 + O2 ↔ SO3
If the equilibrium shifts to the right, the concentration of SO3 will ___________.
SO2 + O2 ↔ SO3
If the equilibrium shifts to the right, the concentration of SO3 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
21.
For the reaction...
SO2 + O2 ↔ SO3
If the concentration of O2 is decreased, the equilibrium of the reaction will shift ___________.
SO2 + O2 ↔ SO3
If the concentration of O2 is decreased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right
d)
neither left nor right
22.
For the reaction...
heat + N2 + O2 ↔ 2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
heat + N2 + O2 ↔ 2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
left and right
d)
neither left nor right
23.
For the reaction...
heat + N2 + O2 ↔ 2NO
If O2 is removed, the concentration of N2 will _______.
heat + N2 + O2 ↔ 2NO
If O2 is removed, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
24.
For the reaction...
heat + N2 + O2 ↔ 2NO
If the heat is removed to the chemical system, the equilibrium will shift _______.
heat + N2 + O2 ↔ 2NO
If the heat is removed to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
both left and right
d)
neither left nor right
25.
For the reaction...
N2 (g) + 3 H2 (g) ↔ 2 NH3 (g)
If the pressure in the system is increased, _______ reaction will be favored.
N2 (g) + 3 H2 (g) ↔ 2 NH3 (g)
If the pressure in the system is increased, _______ reaction will be favored.
a)
the forward
b)
the reverse
c)
neither
26.
Define chemical equilibrium.
a)
A reaction is reversible.
b)
The concentration of the reactants is equal to the concentration of the products.
c)
The rate of a forward reaction is equal to the rate of the reverse reaction.
d)
The reaction stops and no further change in concentration occurs.
27.
What type of reaction can obtain equilibrium?
a)
Double Replacement
b)
Fast Reactions
c)
Reactions with low activation energy
d)
Reversible Reactions
28.
Le Chaltelier's Principle states that if a chemical system at equilibrium is stressed,
a)
the system will adjust to increase the stress
b)
the system will adjust to reduce the stress
c)
the system will not adjust
29.
Why does increased concentration increase the rate of reaction?
a)
the activation energy is lowered
b)
collisions occur with greater energy
c)
the frequency of collisions is increased
30.
Why does temperature increase the rate of reaction?
a)
Increased frequency of collisions
b)
collisions occur with greater energy
c)
the activation energy is lowered
d)
both the frequency and energy of collisions is increased
31.
Why does decreased particle size increase the rate of reaction?
a)
the activation energy is lowered
b)
collisions occur with greater energy
c)
the frequency of collisions is increased
36.
The rate of reaction normally __________
a)
increases a pressure is increased
b)
decreases with the use of a catalyst
c)
decreases as temperature increases
d)
increases as reactant concentration increases
33.
What is the activation energy?
a)
the quantity of heat absorbed in a reaction
b)
the minimum energy needed to begin a reaction
c)
the energy given off after reactants collide.
d)
both the energy and frequeny of collisions in increased
the energy difference between reactants and products
the energy difference between reactants and products
34.
How do catalysts increase the rate of reaction?
a)
The frequency of collisions is the increased
b)
the activation energy is lowered
c)
the energy of collisions is increased
d)
Both the frequency and energy of collisions is increased
35.
How does a catalyst change during a reaction?
a)
It is part of the products
b)
It combines with the reactants
c)
It precipitates
d)
It remains unchanged
36.
The rate of reaction normally __________
a)
increases a pressure is increased
b)
decreases with the use of a catalyst
c)
decreases as temperature increases
d)
increases as reactant concentration increases
37.
During equilibrium, the rates of the forward and the reverse reaction are ________
a)
the same
b)
unequal
c)
unequal for exothermic reactions
d)
unequal for endothermic reactions
38.
What happens to a reaction at equilibrium when more reactant is added?
a)
Equilibrium is shifted to the right
b)
Eqilibrium is shifted to the left
c)
Equilibrium is unchanged
39.
What happens to a reaction at equilibrium when more product is added?
a)
Equilibrium is shifted to the right
b)
Eqilibrium is shifted to the left
c)
Equilibrium is unchanged
40.
What happens to a reaction at equilibrium when product is removed?
a)
Equilibrium is shifted to the right
b)
Eqilibrium is shifted to the left
c)
Equilibrium is unchanged
41.
What happens to a reaction at equilibrium when reactant is removed?
a)
Equilibrium is shifted to the right
b)
Eqilibrium is shifted to the left
c)
Equilibrium is unchanged
42.
What is the Law of Conservation of Mass?
a)
It states that no matter can be created or destroyed.
b)
It states that no energy can be created or destroyed.
c)
It states that matter can be created or destroyed.
d)
It states that no sound can be created or destroyed.
43.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
44.
A + B → AB : is the general form for which reaction type?
a)
Double Replacement
b)
Synthesis
c)
Combustion
d)
Decomposition
45.
Which of the following is an example of synthesis?
a)
Na + Br2 --> NaBr
b)
KClO3 --> KCl + O2
c)
HgO + Cl2-->HgCl + O2
d)
Cl2 + NaBr --> NaCl + Br2
46.
Identify the type of reaction:
Ca + O --> CaO
Ca + O --> CaO
a)
Decomposition
b)
Synthesis
c)
Double Replacement
d)
Combustion
47.
Identify this type of reaction,
Cl2 + 2KI --> I2 + 2KCl
Cl2 + 2KI --> I2 + 2KCl
a)
Synthesis
b)
Single Replacement
c)
Double Replacement
d)
Decomposition
48.
Which chemical reaction forms Carbon Dioxide and Water?
a)
Double Replacement
b)
Single Replacement
c)
Combustion
d)
Decomposition
49.
Which chemical reaction breaks down into 2 substances?
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
50.
Which reaction type is the following: AgF + CaCl2 --> AgCl + CaF2
a)
Decomposition
b)
Single Replacement
c)
Synthesis
d)
Double Replacement
51.
Which reaction type is the following: Na + CaF2 --> Ca + NaF
a)
Decomposition
b)
Single Replacement
c)
Synthesis
d)
Double Replacement
52.
Which of the following is the general formula for a decomposition reaction?
a)
A + B → AB
b)
AB → A + B
c)
AB + C → AC + B
d)
AB + CD → AC + BD
53.
Which reaction type is the following: C5H10O4 + O2 --> CO2 + H2O
a)
Decomposition
b)
Single Replacement
c)
Combustion
d)
Double Replacement
54.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
55.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number to the left of a formula.
56.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO
N2+O2--> _NO
a)
1
b)
2
c)
3
d)
4
57.
What goes in the missing blanks?
SnO2 + __ H2 → Sn + __ H2O
SnO2 + __ H2 → Sn + __ H2O
a)
5
b)
1
c)
3
d)
2
58.
Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe
a)
Yes
b)
No
59.
Balance this equation:
__Li + __Cl2 -> __LiCl
__Li + __Cl2 -> __LiCl
a)
2Li + Cl2 -> 4LiCl2
b)
2Li + Cl2 -> LiCl2
c)
2Li + Cl2 -> 2LiCl
60.
Balance this equation...
HgO --> 2Hg + O2
HgO --> 2Hg + O2
a)
It is balanced
b)
2HgO --> Hg + O2
c)
2HgO --> 2Hg + O2
61.
Which of the following is an unbalanced equation?
a)
CaCO3 --> CaO + CO2
b)
PbO2 + 2H2-->2Pb + H2O
c)
2Na+ 2H2O-->2NaOH + H2
d)
CS2 + 2O2 --> CO2 + 2SO2
62.
Fill in the missing coefficient to balance the equation: Mg + ___ HCl → MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
63.
What type of reaction occurs when ions exchange between two compounds producing either water, a precipitate or a a gas.
a)
combustion
b)
double replacement
c)
single replacment
64.
Acids react with bases to produce ___ and water.
a)
salts
b)
carbon dioxide
c)
oxygen
65.
Hydroxide ions are typically found in
a)
acids
b)
bases
66.
Hydrogen ions are typically found in
a)
acids
b)
bases
67.
Energy is absorbed and stored in the products in
a)
endothermic rxns
b)
exothermic rxns
68.
Energy from reactants is released to the environment.
a)
endothermic rxns
b)
exothermic rxns
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