Chemical equilibria might seem complex, but it's actually about understanding...
Chemistry155 views·Updated 30 Aug 2026·2 pagesUnderstanding Chemical Equilibria
Munsif Shameem@munsifshameem
1
of 2
Understanding Chemical Equilibrium
Ever wondered why some reactions seem to stop halfway? In a closed system (where nothing can escape), reactions reach a fascinating balance point called equilibrium.
Equilibrium occurs when the forward and reverse reaction rates become equal. Think of it like a busy doorway where people enter and leave at exactly the same rate - the number inside stays constant, but there's still movement happening.
Here's what's brilliant: at equilibrium, the concentrations of reactants and products remain constant but aren't necessarily equal. One side might have much more than the other, but the amounts stop changing because the rates balance out.
Industries love this concept because they can manipulate equilibrium to favour their desired products and maximise profits. Catalysts are particularly useful - they speed up both forward and reverse reactions equally, helping you reach equilibrium faster without changing where that balance point sits.
Key Point: Catalysts increase the rate of reaching equilibrium but don't shift the equilibrium position itself.
2
of 2
Shifting Equilibrium - The Big Three Factors
Want to control where your equilibrium sits? You've got three powerful tools: concentration, temperature, and pressure. Mastering these will make you unstoppable in equilibrium problems.
Concentration changes are straightforward. Add more reactant or remove product? The equilibrium shifts right to make more product. Add product or remove reactant? It shifts left. Think of it as the reaction trying to undo whatever you just did.
Temperature effects depend on whether your reaction is endothermic or exothermic. For endothermic reactions, increasing temperature shifts right (more product), whilst decreasing temperature shifts left. Exothermic reactions behave oppositely - higher temperature shifts left, lower temperature shifts right.
Pressure changes only matter when you have different numbers of gas molecules on each side. Increase pressure? The equilibrium shifts towards whichever side has fewer molecules. Decrease pressure? It shifts towards the side with more molecules.
Exam Tip: Remember that equilibrium always tries to counteract whatever change you make to the system - this is Le Chatelier's principle in action.
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Chemistry155 views·Updated 30 Aug 2026·2 pagesUnderstanding Chemical Equilibria
Munsif Shameem@munsifshameem
Chemical equilibria might seem complex, but it's actually about understanding how reactions find their balance point. This knowledge is crucial for industries that need to maximise product yield and will definitely come up in your exams.
1
of 2
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Understanding Chemical Equilibrium
Ever wondered why some reactions seem to stop halfway? In a closed system (where nothing can escape), reactions reach a fascinating balance point called equilibrium.
Equilibrium occurs when the forward and reverse reaction rates become equal. Think of it like a busy doorway where people enter and leave at exactly the same rate - the number inside stays constant, but there's still movement happening.
Here's what's brilliant: at equilibrium, the concentrations of reactants and products remain constant but aren't necessarily equal. One side might have much more than the other, but the amounts stop changing because the rates balance out.
Industries love this concept because they can manipulate equilibrium to favour their desired products and maximise profits. Catalysts are particularly useful - they speed up both forward and reverse reactions equally, helping you reach equilibrium faster without changing where that balance point sits.
Key Point: Catalysts increase the rate of reaching equilibrium but don't shift the equilibrium position itself.
2
of 2Sign up to see the content. It's free!
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Shifting Equilibrium - The Big Three Factors
Want to control where your equilibrium sits? You've got three powerful tools: concentration, temperature, and pressure. Mastering these will make you unstoppable in equilibrium problems.
Concentration changes are straightforward. Add more reactant or remove product? The equilibrium shifts right to make more product. Add product or remove reactant? It shifts left. Think of it as the reaction trying to undo whatever you just did.
Temperature effects depend on whether your reaction is endothermic or exothermic. For endothermic reactions, increasing temperature shifts right (more product), whilst decreasing temperature shifts left. Exothermic reactions behave oppositely - higher temperature shifts left, lower temperature shifts right.
Pressure changes only matter when you have different numbers of gas molecules on each side. Increase pressure? The equilibrium shifts towards whichever side has fewer molecules. Decrease pressure? It shifts towards the side with more molecules.
Exam Tip: Remember that equilibrium always tries to counteract whatever change you make to the system - this is Le Chatelier's principle in action.
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