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Worksheetspractice test on Equilibrium and reaction rates
Total questions: 35
Worksheet time: 49mins
Name
Class
Date
1.
Rate of chemical reaction means
a)
amount of product formed
b)
speed of reaction
c)
concentration of reacting particles
d)
combining reactants with products
2.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
3.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Neutralise the reaction
d)
increase collision between the particles thus increasing the rate.
4.
Reactions that give out heat to the surrounding are classified as one of the following:
a)
Spontaneous
b)
Sluggish
c)
Exothermic
d)
Endothermic
5.
Why don't all collisions between particles cause a reaction?
a)
the particles also need to collide with a catalyst
b)
not all the particles collide with enough energy
c)
not all the particles collide at a high enough temperature
d)
the particles need to collide with each other twice
6.
B represents
a)
energy absorbed
b)
energy released
c)
activation energy
7.
A chemical reaction that requires energy to happen
a)
Exothermic
b)
Endothermic
c)
Explosive
d)
Hot reaction
8.
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
9.
When writing an endothermic reaction, heat energy is stated as
a)
product
b)
catalyst
c)
reactant
10.
An exothermic reaction is allowed to reach equilibrium. If heat energy is then removed, the equilibrium will shift
a)
toward the middle
b)
toward the reactant side
c)
toward the product side
11.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
12.
For the reaction...
SO2(g) + O2(g) <−> SO3(g)
If the concentration of SO2(g) is increased, the equilibrium of the reaction will ___________.
SO2(g) + O2(g) <−> SO3(g)
If the concentration of SO2(g) is increased, the equilibrium of the reaction will ___________.
a)
shift to the left
b)
shift to the right
c)
not shift
13.
For the reaction...
SO2(g) + O2(g) <−> SO3(g)
If the equilibrium shifts to the right, the concentration of O2(g) will ___________.
SO2(g) + O2(g) <−> SO3(g)
If the equilibrium shifts to the right, the concentration of O2(g) will ___________.
a)
increase
b)
decrease
c)
remain the same
14.
For the reaction...
N2 (g) + 3 H2 (g) <−> 2 NH3 (g)
If the pressure in the system is increased, the reaction will __________________.
N2 (g) + 3 H2 (g) <−> 2 NH3 (g)
If the pressure in the system is increased, the reaction will __________________.
a)
shift to the left
b)
shift to the right
c)
not shift
15.
The three factors that affect the equilibrium of a reaction are temperature, pressure and __________.
a)
energy
b)
concentration
c)
enthalpy
d)
ice
16.
2SO2(g)+O2(g)⇌2SO3(g)
Removing O2(g) will
Removing O2(g) will
a)
shift equilibrium right
b)
shift equilibrium left
c)
decrease temperature
d)
have no change
17.
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.
18.
N2O4(g) ↔ 2 NO2(g)
What is the concentration equilibrium constant expression?
What is the concentration equilibrium constant expression?
a)
Kc = [NO2]2/[N2O4]
b)
Kc = [N2O4]/[NO2]2
c)
Kc = [N2O4]2/[NO2]
d)
Kc = [NO2]/[N2O4]2
19.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
20.
What is the equilibrium-constant expression for
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
a)
Kc= [CO][H2O] / [CO2][H2]
b)
Kc= [CO2][H2] / [CO]
c)
Kc= [CO2][H2] / [CO][H2O]
d)
Kc= [CO] / [CO2][H2]
21.
What is the equilibrium expression for:
Fe3O4(s) + 4H2(g) <--> 3Fe(s) + 4H2O(g)
Fe3O4(s) + 4H2(g) <--> 3Fe(s) + 4H2O(g)
a)
([Fe]3[H2O]4 ) / ([Fe3O4][H2]4)
b)
([Fe3O4][H2]4)/ ([Fe]3[H2O]4)
c)
[H2O]4 / [H2]4
d)
([Fe][H2O]) / ([Fe3O4][H2])
22.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
23.
Keq < 1
a)
There are more products than reactants when the reaction reached equilibrium.
b)
There are more reactant than products when the reaction reached equilibrium.
c)
The amount of reactants is equal to the amount of products.
24.
What kind of reaction is this?
a)
Endothermic
b)
Exothermic
c)
Equilibrium
d)
Can not be determined
25.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
26.
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
27.
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
28.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction.
a)
catalyst
b)
product
c)
reactant
d)
solute
29.
Smaller particle size allows for a _________ surface area to be exposed for the reaction.
a)
larger
b)
smaller
30.
Increasing the temperature will increase the kinetic energy of particles, therefore increasing the collisions between particles.
a)
false
b)
true
31.
In an endothermic reaction the products have
a)
more energy than the reactants
b)
less energy than the reactants
c)
the same energy as the reactants
d)
no energy
32.
C represents
a)
energy absorbed
b)
energy released
c)
activation energy
33.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
34.
CO (g) + 3H2 (g) <----> CH4 (g) + 3H2O (g) At equilibrium [CO] = 4.0 M. [H2] = 2.8 M. [CH4] = .75 M, and [H2O] = .12M. Find the Keq constant.
a)
Keq =1.65 x 104
b)
Keq = 6.5 x 10-6
c)
Keq = 1.48 x 10-5
d)
Keq = 3.2 x 105
35.
For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentration are as shown?
A (g) + 2B (g) <-----> C (g)
equilibrium concentrations (M). A = 4.5 x 10-5 B = 2.2 x 10-2
C = 9.4 x 10-3
Find Keq:
a)
.22
b)
9.9
c)
4.3 x 105
d)
2.3 x 108
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