Catalysts and Activation Energy Worksheet

Question 1

Which change explains why a catalyst can increase reaction rate?

1. It provides a pathway with a lower activation energy.
2. It increases the number of atoms in the reactants.
3. It always increases the net energy released per mole.
4. It removes the need for reactant particles to interact.

Question 2

Two pathways connect the same reactants and products, but one has a lower peak. Explain why they have the same net energy change.

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Question 3

Reactants have a potential energy of 25 kJ/mol and a pathway peaks at 85 kJ/mol. Calculate the forward activation energy.

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Question 4

Which statement describes the effect of a catalyst at a fixed temperature?

1. It raises the average kinetic energy of all reactants.
2. It raises the minimum energy needed for reaction.
3. It lets more particles reach the energy threshold for reaction.
4. It makes every collision produce a reaction.

Question 5

Which pathway represents the catalyzed reaction?

1. Path A, because it has a higher peak.
2. Path B, because it has a lower peak.
3. Path A, because it has a lower product energy.
4. Both, because they have identical barriers.

Question 6

Use the graph to calculate the forward activation energy of each path.

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Question 7

What is the net energy change for the reaction in the graph?

1. −80 kJ/mol
2. −20 kJ/mol
3. +20 kJ/mol
4. +60 kJ/mol

Question 8

Which path also has a smaller activation energy for the reverse reaction? Use the graph to justify your answer.

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