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⚗️ How Chemical Equilibria Shift

Learn how concentration, pressure, temperature, inert gases, and catalysts affect a chemical equilibrium—and when the reaction quotient can check your prediction.

lessons

~10 min

to learn

🔬 Science

subject

Adults

level

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What you’ll learn

Core equilibrium ideasDistinguish dynamic equilibrium from a stopped reaction and predict how concentration changes alter direction without changing K at fixed temperature.Equilibrium means equal opposing rates and constant concentrations, not equal amounts. A concentration disturbance changes Q and produces a net reaction until Q returns to K.
Stresses and responsesPredict the effects of gas pressure, temperature, catalysts, and inert gases while stating the condition that makes each prediction valid.Compression can favor fewer gas moles, temperature favors the endothermic direction and changes K, catalysts shorten the wait without changing position, and inert gases shift only when the constraint changes reacting partial pressures.
Apply and explainUse Q versus K and the Haber process to turn an equilibrium prediction into a concise, properly qualified explanation.Q checks direction after a disturbance; industrial ammonia production combines pressure, temperature, catalysis, removal, and recycling because yield and speed pull in different directions.

Questions this course answers

What is equal at dynamic equilibrium?

Equilibrium is dynamic: opposing rates are equal while concentrations remain constant.

What happens when a reactant is added?

The net reaction initially favors the direction that consumes the added reactant.

When does pressure favor fewer gas moles?

Decreasing volume raises pressure and favors the side with fewer gaseous particles when the gas-mole counts differ.

Which change alters K?

The equilibrium constant changes with temperature; the other changes do not change K under the stated conditions.

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