WorksheetsEquilibrium Quiz
Total questions: 15
Worksheet time: 16mins
Explain the meaning of the term 'reversible reaction'
Explain the meaning of the term 'irreversible reaction'
A chemical reaction is in equilibrium when:
The forward and reverse reaction have stopped
The equilibrium constant equals 1
The forward and reverse reaction rates are equal
No reactants remain
Consider the following reaction in equilibrium:
2 C(s)+O2(g) ↔2 CO(g)
What is the equilibrium expression?
[O2][CO]2
[O2][C]2[CO]2
[O2][2C]2[CO]
[O2][CO]
Le Chatelier's Principle states that:
At equilibrium, the forward and reverse reaction rates are equal
Stresses include changes in concentration, pressure, and temperature
To relieve stress, solids and liquids are omitted from the equilibrium constant expression
Chemical equilibria respond to reduce applied stress
In an exothermic reaction, where heat is released, heat is considered a:
Reactant
Product
It is not considered part of the reaction
A certain reaction has an equilibrium constant of K = 0.0000578
This reaction favors the products
This reaction favors the reactants
This reaction is equally favored in both directions
This reaction is bad
When is the rate of the forward reaction the greatest?
At equilibrium
In the beginning, when there are more reactants than products
In the end, when there are more products than reactants
Never
What is static equilibrium?
The same thing as static equilibrium.
The static on the tv.
Opposite reactions creating no net change.
When something comes to a stop.
How is chemical equilibrium different from static equilibrium?
They are different
Chemical equilibrium is when a reversible reaction stops completely, and static equilibrium is when a reversible reaction has equal rates of the forward and reverse reaction.
Chemical equilibrium is when the rates of two opposite events are equal. Something is happening but there is no change. Static equilibrium is when something stops.
There is no difference between them
Consider this reversible reaction in equilibrium:
2 NO2(g) ↔N2O4(g) + Heat
How will the equilibrium shift if the temperature is increased (heat is added)?
The reaction will shift left to make more reactants.
The reaction will shift right to make more products
Nothing will change
The reaction will become cooler
Consider the reaction:
2 NO2(g) ↔N2O4(g) + Heat
Where will the equilibrium shift of NO2 is removed?
No change will occur
The reaction will shift right to make more products
The reaction will shift left to make more reactants
Consider the following reaction:
2 NO2(g) ↔N2O4(g) + Heat
Where will the equilibrium shift if N2O4 is added?
The reaction will shift right (to products)
The reaction will shift left (to reactants)
No change
If a reversible reaction in equilibrium has equal amounts of gas on both sides, what will happen if the pressure is increased (aka the space is decreased)?
To the side with less gas.
To the sides will more gas.
No change. There is no favored way to fix the equilibrium.
What is an example of something going back to equilibrium? Doesn't have to do with chemistry.
