WorksheetsChemical Reaction Rates and Equilibrium
Total questions: 21
Worksheet time: 12mins
An increase in temperature will cause:
Increased reaction rate
No change
Decreased reaction rate
An increase in volume of gases will cause:
Increased reaction rate
No change
Decreased reaction rate
An increase in pressure of gases will cause:
Increased reaction rate
No change
Decreased reaction rate
An increase in concentration of a solution will cause:
Increased reaction rate
No change
Decreased reaction rate
An increase in surface area of reactants will cause:
Increased reaction rate
No change
Decreased reaction rate
HCl is reacted with Zn to form ZnCl2 and H2 gas. The concentration of HCl is increased from 0.5 mol/L to 2 mol/L. What happens to the rate of reaction?
It will increase
It will stay the same
It will decrease
A reaction mixture of NaOH and formaldehyde is cooled from 80oC to 0oC. What happens to the rate of reaction?
It will increase
It will stay the same
It will decrease
H2 gas and O2 gas are reacting together to form water in a sealed container. The volume of the container is expanded from 2L to 10L. What will happen to the rate of reaction?
It will increase
It will stay the same
It will decrease
Magnesium can combust in air to form magnesium oxide. If we use a fine powder of Mg instead of a solid block, what will happen to the rate of reaction?
It will increase
It will stay the same
It will decrease
The Haber process reacts together H2 and N2 gases to form NH3. What will happen to the rate of reaction if we increase the pressure of these gases?
It will increase
It will stay the same
It will decrease
Collision theory states that:
atoms, ions, and molecules must collide with enough energy to react
atoms, ions, and molecules must collide to react
atoms, ions, and molecules must have enough energy to react
atoms, ions, and molecules can react at any time, doesn't matter how close they are or how much energy they have.
How do catalysts work to affect rate of reaction?
They increase the energy of the reactants
They increase the number of collisions
They lower the activation energy of the reaction
They increase the activation energy of the reaction
What can be done to slow down the rate of reaction?
Add a catalyst
Increasing temperature
Add an inhibitor
Increase pressure
What can be added to food to slow down decomposition reactions (rotting)?
Catalyst
Inhibitor
Temperature
Pressure
A reversible reaction is at equilibrium. This means that _______.
There are equal amounts of reactants and products
The forwards and backwards reactions are happening at the same rate
The reaction has now completely stopped
In a reversible reaction, if the forwards reaction is exergonic then the backwards reaction is _____.
exergonic
endergonic
we can't tell from this information
A reversible reaction is at equilibrium. The temperature of the reaction is increased. How will the equilibrium shift?
The exothermic reaction will speed up
The endothermic reaction will speed up
The reaction will not change
Consider the following reaction: N2O4 (g) ↔ 2NO2 (g).
If we increase the pressure on the reaction, which way will the equilibrium shift?
To the left, as this will decrease the number of molecules of gas and reduce pressure.
To the right, as this will decrease the number of molecules of gas and reduce pressure.
To the left, as this will increase the number of molecules of gas and increase pressure.
To the right, as this will increase the number of molecules of gas and increase pressure.
Consider the Haber process shown here. If we increase the temperature of the reaction, what will happen to the equilibrium?
It will move to the right and produce more ammonia (NH3)
It will move to the left and produce more ammonia (NH3)
It will move to the right and produce more H2 and N2
It will move to the left and produce more H2 and N2
Le Chatelier's principle states that if we change the conditions of a reversible reaction, ________________.
The equilibrium will shift to increase that change
The equilibrium will shift to oppose that change
The equilibrium will not change
Consider this reversible reaction at equilibrium. If you increase the concentration of C and D, what will happen to the equilibrium?
It will shift to the left to produce more A and B
It will shift to the right to produce more C and D
The equilibrium won't change
We need more information to answer this
