Chemistry · GCSE · Rates & Equilibrium

Changing concentration at equilibrium

Changing concentration at equilibriumFree4:06Heddy Score 3 of 7, below the standard
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What you need to know

  • In a reversible reaction the products can turn back into the reactants, shown with a double arrow.
  • At equilibrium the forward and reverse reactions keep going at the same rate, so the amounts no longer change (dynamic equilibrium).
  • Le Chatelier's principle: if conditions change, the equilibrium shifts to counteract the change.
  • Adding more of a reactant (more nitrogen in the Haber process) or removing a product (ammonia) shifts the equilibrium to the right, making more product.

In this clip

Runs 4:06, from 1:25 to 5:31 of the full video.

Heddy Score3/7, Below the standard
See the seven stars
  • Trusted source · passed. The creator's own upload, live and playable here.
  • On the map · not judged yet. A teacher watched it: it mainly teaches this map topic.
  • Spec-true · not judged yet. Accurate, and right for the current UK specification.
  • Focused · passed. One idea, short enough to watch in one go.
  • Accessible · passed. Good captions, clear sound and pictures.
  • Safe for children · not judged yet. Right for 11 to 16 year olds, with no sales pitch.
  • Proven · not judged yet. Earned from our students: they learn from it, find it helpful and watch it to the end.
★ passed · ☆ pending · ✕ failed
Our students

Not enough students yet

Our own students' answers. These are what move ★7 Proven.
On YouTube

2.77M views · 33.5K likes · CrashCourse 17.3M subscribers

As reported by YouTube on 2026-11-02. Not part of the Heddy Score.
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Why we picked it

Explains dynamic equilibrium and Le Chatelier's principle with the Haber process, then makes the temperature effect visible with a colour-changing demonstration.

CrashCourse on YouTubechecked 2026-10-22

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