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4 Feb 2026

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2 pages

Understanding Chemical Equilibria: A Guide

Aisha Abdullahi

@aishaabdullahi_deom

Chemical equilibria might seem complex, but they're actually quite logical... Show more

$Equilibria. Reversible reactions. ↳ Reactions go forward & Backward. ($\rightleftharpoons$) ↳ If its exothermic on one side, its endothermi$

Reversible Reactions and Le Chatelier's Principle

Ever noticed how some chemical reactions seem to go both ways? That's because reversible reactions can proceed forward and backward simultaneously, creating a dynamic balance. Here's the key insight: if a reaction releases energy (exothermic) in one direction, it absorbs the exact same amount of energy (endothermic) when going the opposite way.

Le Chatelier's Principle is your best mate for predicting what happens when you mess with this balance. The rule is simple: disturb an equilibrium system, and it'll fight back by shifting to counteract your change.

When you increase concentration of any substance, the equilibrium shifts away from that substance to reduce its concentration. It's like the reaction is trying to use up the excess you've added.

For pressure changes, remember that equilibrium shifts towards the side with fewer gas molecules when pressure increases. The system literally tries to take up less space to reduce the pressure you've applied.

Quick Tip: Temperature changes are trickier - increasing temperature shifts the equilibrium towards the endothermic direction, as the system tries to absorb that extra heat energy.

$Equilibria. Reversible reactions. ↳ Reactions go forward & Backward. ($\rightleftharpoons$) ↳ If its exothermic on one side, its endothermi$

Catalysts and Equilibrium Constants

Here's something that catches many students out: catalysts don't affect equilibrium position at all. They're like a fair referee - they speed up both the forward and backward reactions equally, helping you reach equilibrium faster without favouring either side.

The equilibrium constant (Kc) is your mathematical tool for describing equilibrium quantitatively. For any reaction aA + bB ⇌ cC + dD, you calculate it as: Kc = [Products]/[Reactants], where each concentration is raised to the power of its coefficient in the balanced equation.

Understanding Kc values helps predict reaction behaviour. A large Kc means products are favoured at equilibrium, whilst a small Kc indicates reactants dominate the mixture.

Exam Insight: Remember that Kc only changes with temperature - not concentration, pressure, or catalysts. This is a common exam question that trips up many students!

The square brackets [X] represent concentration in mol dm⁻³, and you'll need to use the balanced chemical equation to get the correct powers for your calculation.

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197

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4 Feb 2026

•

2 pages

Understanding Chemical Equilibria: A Guide

Aisha Abdullahi

@aishaabdullahi_deom

Chemical equilibria might seem complex, but they're actually quite logical once you understand the basic principles. Think of it like a perfectly balanced see-saw that adjusts itself whenever someone tries to tip it - that's exactly how chemical reactions behave... Show more

$Equilibria. Reversible reactions. ↳ Reactions go forward & Backward. ($\rightleftharpoons$) ↳ If its exothermic on one side, its endothermi$

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Reversible Reactions and Le Chatelier's Principle

When you increase concentration of any substance, the equilibrium shifts away from that substance to reduce its concentration. It's like the reaction is trying to use up the excess you've added.

Quick Tip: Temperature changes are trickier - increasing temperature shifts the equilibrium towards the endothermic direction, as the system tries to absorb that extra heat energy.

$Equilibria. Reversible reactions. ↳ Reactions go forward & Backward. ($\rightleftharpoons$) ↳ If its exothermic on one side, its endothermi$

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Catalysts and Equilibrium Constants

Understanding Kc values helps predict reaction behaviour. A large Kc means products are favoured at equilibrium, whilst a small Kc indicates reactants dominate the mixture.

Exam Insight: Remember that Kc only changes with temperature - not concentration, pressure, or catalysts. This is a common exam question that trips up many students!

The square brackets [X] represent concentration in mol dm⁻³, and you'll need to use the balanced chemical equation to get the correct powers for your calculation.