WorksheetsLeChatelier's Principle
Total questions: 18
Worksheet time: 15mins
Name
Class
Date
1.
For the equilibrium reaction
2NH3(g) + 22 kJ ↔ N2(g) + 3H2(g),
which of the following changes would result in the formation of more N2 and H2 at equilibrium?
2NH3(g) + 22 kJ ↔ N2(g) + 3H2(g),
which of the following changes would result in the formation of more N2 and H2 at equilibrium?
a)
increasing temperature
b)
adding N2
c)
removing NH3
2.
2.In the Haber process, gaseous ammonia is produced on an industrial scale by combining nitrogen and hydrogen gases, according to this equation:
N2(g) + 3H2(g) ↔ 2NH3(g)
The process is exothermic. Which of the following actions will shift the reaction in the forward (product) direction?
N2(g) + 3H2(g) ↔ 2NH3(g)
The process is exothermic. Which of the following actions will shift the reaction in the forward (product) direction?
a)
Increase the temperature of the reaction.
b)
Reduce ammonia (NH3) concentration by removing ammonia from the reaction chamber.
c)
Reduce hydrogen concentration by reducing the amount of hydrogen in the reaction chamber.
3.
The principle that states that if a system at equilibrium is disturbed, the reaction will proceed in one direction or another in order to reestablish equilibrium, is known as:
a)
The principle of equilibrium
b)
Priestley’s principle
c)
Le Chatelier’s principle
d)
Faraday’s principle
4.
What is the effect of changing the concentration of one of the reactants in an equation at equilibrium?
a)
the reaction will stay at equilibrium
b)
the reaction will stop
c)
the reaction will continue to completion
d)
the reaction will shift to re-establish equilibrium.
5.
A system at equilibrium means it is still reacting.
a)
True
b)
False
6.
For an endothermic reaction, heat can be thought of as:
a)
a reactant
b)
a product
c)
either it has no effect
d)
neither it effects both sides equally.
7.
Increasing the concentration of the reactants will:
a)
shift the reaction to the left towards the reactants, making more of the reactants.
b)
shift the equilibrium to the right towards the products, making more of the product.
c)
Have no effect on equilibrium.
8.
Increasing the temperature of an exothermic reaction will:
a)
shift the reaction to the left towards the reactants, making more of the reactants.
b)
shift the equilibrium to the right towards the products, making more of the product.
c)
Have no effect on equilibrium.
9.
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
10.
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
11.
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
12.
For the reaction...
heat + N2 + O2 <−> 2NO
If NO is removed from the system, the concentration of N2 will _______.
heat + N2 + O2 <−> 2NO
If NO is removed from the system, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
13.
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
14.
For the reaction...
H2 (g) + Cl2 (g) <−> 2HCl (g) + heat
If the temperature is cooled, the _________ reaction will be favored.
H2 (g) + Cl2 (g) <−> 2HCl (g) + heat
If the temperature is cooled, the _________ reaction will be favored.
a)
forward
b)
reverse
c)
forward and reverse
15.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
16.
If the enthalpy ter (ΔH) is negative the reaction is ____.
a)
Endothermic
b)
Exothermic
c)
Neutral
17.
What type of reaction is this?
a)
Exothermic
b)
Endothermic
c)
Energy Producing
d)
No way to tell
18.
How do you calculate the Enthalpy of Reaction?
a)
ΔH = ΔHproducts - ΔHreactants
b)
ΔG = ΔH -TΔS
c)
ΔT = q / mC
d)
E = mc2
100 %
