Learning objective
Explain that increasing gas pressure increases collision frequency.
Read the explanation, check the common trap, then practise with flashcards and questions.
At a glance
0
Flashcards
0
Questions
Topic
Rate of reaction
Subtopic
Collision theory and activation energy
Study support
Understand this objective
Quick explanation
Explain that increasing gas pressure increases collision frequency
- This point belongs to Rate of reaction, especially Collision theory and activation energy.
- You need to be able to explain that increasing gas pressure increases collision frequency.
- The key ideas to know are pressure.
- Use the linked flashcards and practice questions to check recall, then practise applying the idea in an exam-style answer.
Key concepts
Why it matters
This objective helps connect Collision theory and activation energy to exam-style questions, flashcards, and revision notes for Rate of reaction.
Quick student answer
How do you explain increasing gas pressure increases collision frequency?
Direct answer
In Chemistry, this page helps you answer questions about increasing gas pressure increases collision frequency within Rate of reaction. Focus on the key process, correct scientific terms, and how the idea links to exam-style questions. Key terms to check are collision frequency and gas pressure.
Key terms
- collision frequency: the number of collisions between particles in a given time period, which affects the rate of reaction. In AQA GCSE Chemistry 8462, use this term specifically when explaining rate of reaction, collision theory, reversible reactions, equilibrium, catalysts, graph gradients, or Le Chatelier's principle.
- gas pressure: the force exerted by gas particles when they collide with the walls of their container, influencing the rate of reaction. In AQA GCSE Chemistry 8462, use this term specifically when explaining rate of reaction, collision theory, reversible reactions, equilibrium, catalysts, graph gradients, or Le Chatelier's principle.
Common trap
Misunderstanding Pressure Effects: Remember that increasing pressure compresses the gas, leading to more frequent collisions between particles, not higher energy.
Related questions
Try this as a practice card
Question 1 of 4
Choose an answer, get feedback, then move sideways through the set.
Flashcard prompts
Flip through the key recall cards
Flashcard 1 of 4
Practise next
Revision tools
Choose how to practise
Flashcards0 linked cards
Practice Questions0 linked questions
Revision notestopic notes
Open the full topic revision notes when you are ready to review this objective in context.
Open revision notesRelated learning objectives
- Define rate of reaction as the speed at which reactants are used up or products are formed.
Calculating rates of reactions
- Calculate mean rate of reaction using quantity of reactant used divided by time taken. (MS 1a)
Calculating rates of reactions
- Calculate mean rate of reaction using quantity of product formed divided by time taken. (MS 1a)
Calculating rates of reactions
- Use units such as g/s, cm3/s or mol/s for rate of reaction calculations.
Calculating rates of reactions
- Interpret rate data from tables and graphs.
Calculating rates of reactions