Chemical equilibrium laboratory
Compare Q with K and apply concentration, pressure, temperature and catalyst stresses.
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Explanation mode
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Description of this simulation
Q = 1.000, K = 4.000; the mixture responds in the forward direction and the selected stress predicts a forward shift.
Quick test · 3 questions
- Q
- 1.0000
- K
- 4.0000
- Net reaction direction
- forward
- Predicted equilibrium shift
- forward
- Does this stress change K?
- No
Learning guide
- Learning objective
- Use Q and K to predict direction, then distinguish composition changes from changes to K.
- Core equation
- Q = [products]^ν/[reactants]^ν; compare Q with K
- Why the result changes
- The system consumes an imposed concentration or pressure change; only temperature changes the equilibrium constant.
- Try this challenge
- Add a catalyst and verify that neither the equilibrium position nor K changes.
- Sources
- IUPAC Gold Book; Atkins' Physical Chemistry
What this model shows — and what it simplifies
Educational ModelQ is calculated from the current composition; K belongs to a stated reaction at a stated temperature.
Where do we see this in real life?
Industrial reactors balance equilibrium yield against rate, energy use and safe operating pressure.
Explain this result
Scientific review record
Building- Module version
- v1 bundled
- Published
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- Last reviewed
- Not yet verified
- Academic level
- School
- Reviewer
- Not publicly assigned
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