Starter track
Step 1 of 20 / 2 completeRates and Equilibrium
Next after this: Dynamic Equilibrium / Le Chatelier's Principle.
1. Reaction Rate / Collision Theory2. Dynamic Equilibrium / Le Chatelier's Principle
This concept is the track start.
Concept module
Reaction Rate / Collision Theory
Keep one chemistry box visible so temperature, concentration, activation threshold, and catalysts can be read as changes in successful collisions instead of chemistry slogans.
Interactive lab
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Stable links
Why it behaves this way
Explanation
Reaction rate becomes easier to trust when the collision story stays visible. This module keeps one particle box, one activation threshold, and one live rate readout together so temperature, concentration, and the barrier all stay attached to the same cause-and-effect bench.
The key distinction is that more collisions are not automatically more reaction. Concentration mostly changes how often particles meet, while temperature and barrier changes decide how many of those meetings are energetic enough to succeed.
Key ideas
01Reaction rate depends on successful collisions, not just on how often particles hit each other.
02Raising temperature increases both how often particles collide and how likely those collisions are to clear the barrier.
03A catalyst changes the barrier story without having to make the particles hotter.
Frozen walkthrough
Step through the frozen example
Frozen walkthrough
Use the current chemistry bench instead of a detached worksheet. The same controls drive the particle box, the response graphs, and these substitutions.
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View plansFrozen valuesUsing frozen parameters
For the current mixture, how do all collisions and successful collisions differ?
Temperature
3.1
Concentration
1.4
Activation threshold
2.8
1. Read how often the particles collide
At the current temperature and concentration, the box makes about 32.73 collision attempts each second.
2. Read how many of those hits clear the threshold
Only about 37.46% of those collisions clear the effective barrier.
3. Turn that into a reaction rate
That leaves about 12.26 successful collisions each second and about 20.47 unsuccessful ones.
Current successful-collision rate
The box is busy, but most hits still fail the barrier test, so all-collision count and successful-collision rate need to be kept separate.
Common misconception
If concentration increases, then the reaction must speed up because every extra collision is automatically a successful one.
Higher concentration mainly creates more collision attempts.
Whether those attempts become reactions still depends on how many collisions clear the activation threshold.
Mini challenge
Make the reaction noticeably faster without relying on a very crowded box.
Make a prediction before you reveal the next step.
Decide whether you should change the collision frequency, the barrier, or the successful fraction before you try it.
Check your reasoning against the live bench.
You need a setup where a decent share of collisions clears the barrier even though concentration stays moderate.
That is the cleanest way to separate more collisions from more successful collisions. The rate rises because the successful fraction improves, not because the box is simply packed.
Quick test
Misconception check
Question 1 of 3
Answer from the live chemistry story, not from a memorized slogan.
Which statement is the most honest one?
Use the live bench to test the result before moving on.
Accessibility
The simulation shows a particle box with reactants moving inside it, plus visible cues for all collisions, successful collisions, and the barrier-clearing share. Sliders change temperature, concentration, and activation threshold, and a toggle applies a catalyst.
A readout card reports the current temperature, concentration, threshold, successful share, and successful-collision rate so the learner can compare the visual box with the graph response.
Graph summary
One graph compares all collision attempts with successful collisions as temperature changes, a second does the same for concentration, and a third shows the successful fraction against temperature.
Graph hover, compare mode, and the shared overlays all stay tied to the same chemistry bench instead of opening a separate view.
Keep the chemistry branch moving
Keep this idea moving
Open the next concept, route, or track only when you want the current model to widen into a larger branch.
Carry the collision story into a reversible system that re-balancesRates and Equilibrium
Dynamic Equilibrium / Le Chatelier's Principle
Watch a reversible chemistry bench keep changing microscopically while the mixture settles toward a new balance after each disturbance.
Useful comparisonThermodynamics
Temperature and Internal Energy
Compare average particle motion with whole-sample energy, vary amount and heating, and see why a phase-change shelf breaks naive temperature-only reasoning on one compact thermal bench.
Useful comparisonThermodynamics
Ideal Gas Law and Kinetic Theory
Connect pressure, volume, temperature, and particle number on one bounded particle box, then read the same pressure changes back as changes in particle speed and wall-collision rate.