Catalysts and Activation Energy Flashcards

1️⃣ Familiarise yourself with the flashcards:

  • Look through all the flashcards to see what's on both sides.
  • Make sure you understand the information on each card. If something's unclear, click the link to the revision notes at the bottom of the page for more details.

2️⃣ Test yourself:

  • Look at the question or prompt on each card and try to remember the answer before flipping it over.
  • Check the answer and make a note of any cards you find challenging and need to go over more.

3️⃣ Consistently Review and Practice:

  • Use spaced repetition: spend more time on the cards you struggle with and go over them more often.
  • Regularly review all the flashcards to help you better understand and retain the information over time.

Note: We may include questions that have multiple correct answers. It's useful to remember specific examples to understand these concepts better.

PERSONALISED 1-TO-1 TUTORING

Need more help on this topic? Get 1-to-1 support

Get support with clear explanations, practice and feedback (Ages 5 to 16).

  • DBS-checked tutors
  • Flexible times
  • Parents can be updated

Want an ad-free experience? Subscribe to remove ads

What is activation energy?

It is the minimum energy that particles must have to react when they collide.

What is a catalyst?

A catalyst is a substance that speeds up a chemical reaction without being used up.

How does a catalyst change the activation energy of a reaction?

It provides a different reaction pathway with a lower activation energy.

Why does lowering the activation energy make a reaction faster?

More particles then have enough energy, so more collisions are successful each second.

Is a catalyst used up during a reaction?

No. It is not used up and can be used again and again.

Does a catalyst change how much energy is released or taken in by a reaction?

No. It only changes the rate of reaction, not the total energy change.

On an energy profile diagram, how does a catalysed reaction look different?

The peak is lower, so the activation energy arrow is smaller than for the uncatalysed reaction.

Why are catalysts useful in industry?

They let reactions run faster at lower temperatures, saving energy, money and reducing carbon dioxide emissions.

Why do different reactions often need different catalysts?

Because most catalysts only work for certain reactions, as their surface or structure suits only those reactants.

Give one example of a catalyst and the reaction it speeds up.

Iron is a catalyst in the Haber process, where nitrogen and hydrogen react to make ammonia.