Linked from

The 32 pages that link to Le Chatelier's principle, each with the reason it gives.

• Chemical equilibriumRelated: It gives a qualitative way to predict responses to concentration, pressure, or temperature changes.

• EsterificationRelated: Removing water or using excess alcohol shifts the reversible reaction toward ester products.

• Haber–Bosch processRelated: Ammonia formation shrinks gas volume, so high pressure drives the equilibrium toward product.

• Acid–base equilibriumRelated: It predicts how added acid, base, or other species shifts proton-transfer balance.

• Fritz HaberRelated: High pressure favors the ammonia side because its formation reduces the number of gas molecules.

• Haber processRelated: High pressure favors ammonia because its formation reduces the number of gas molecules.

• Chemical thermodynamicsRelated: Thermodynamic equilibrium calculations give quantitative form to these shifts.

• TransesterificationRelated: Excess alcohol or removal of products can drive this reversible reaction toward biodiesel.

• ChromateRelated: It predicts the direction of chromate–dichromate shifts after changing acidity.

• Dynamic equilibriumRelated: A disturbance changes rates unequally at first, driving the system toward a new equilibrium.

• Weak acidRelated: Adding the conjugate base shifts a weak acid’s dissociation equilibrium toward its undissociated form.

• Contact processRelated: It explains why temperature and pressure choices balance conversion, rate, and cost.

• Common-ion effectRelated: Adding a shared ion changes concentration, prompting the equilibrium shift behind the effect.

• Reaction quotientRelated: Changes in composition alter Q and prompt a shift toward a new equilibrium.

• Van ’t Hoff equationRelated: The equation quantifies the temperature shifts that the principle predicts qualitatively.

• Ammonium chlorideRelated: It helps explain shifts in the ammonium–ammonia equilibrium as conditions change.

• Hydration reactionRelated: Changing water concentration can shift the balance between a compound and its hydrate.

• Ammonia synthesisRelated: High pressure and lower temperature favor ammonia at equilibrium, though kinetics constrain operation.

• Fischer esterificationRelated: Excess alcohol or removal of water drives ester formation forward.

• Water–gas shift reactionRelated: Adding steam or removing products shifts the reaction toward hydrogen and carbon dioxide.

• pH indicatorRelated: Adding or removing protons shifts the indicator equilibrium toward a different form.

• Reversible reactionRelated: Changes to a reversible reaction's conditions alter its equilibrium composition.

• Sodium chromateRelated: It explains the pH-dependent chromate–dichromate balance.

• Dean–Stark apparatusRelated: Removing product water can shift a reversible condensation toward products.

• Dinitrogen tetroxideRelated: It predicts how heating or compression changes the NO₂–N₂O₄ mixture.

• Cobalt(II) chlorideRelated: Adding chloride or water can shift cobalt’s coordination equilibrium and its color.

• Potassium thiocyanateRelated: Adding thiocyanate shifts the iron(III) complex equilibrium toward its red-colored products.

• Chromate and dichromateRelated: It predicts the direction of the color-changing equilibrium after acid or base is added.

• Sodium formateRelated: It helps explain the effect of temperature and pressure on reversible formate decomposition reactions.