Chemical equilibria and Le Chatelier's principle (3.1.6.1) | AQA A-level Chemistry - (7405) | KnowledgeSet

Chemical equilibria and Le Chatelier's principle

Chemistry · A-Level · AQA · AQA A-level Chemistry - (7405) · Specification point · 3.1.6.1 · Physical chemistry · Chemical equilibria, Le Chatelier’s principle and Kc

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3.1.6.1 Chemical equilibria and Le Chatelier's principle

Content	Opportunities for skills development
$Many chemical reactions are reversible. In a reversible reaction at equilibrium: forward and reverse reactions proceed at equal rates the concentrations of reactants and products remain constant Le Chatelier’s principle. Le Chatelier's principle can be used to predict the effects of changes in temperature, pressure and concentration on the position of equilibrium in homogeneous reactions. A catalyst does not affect the position of equilibrium. Students should be able to: use Le Chatelier’s principle to predict qualitatively the effect of changes in temperature, pressure and concentration on the position of equilibrium explain why, for a reversible reaction used in an industrial process, a compromise temperature and pressure may be used.$	$PS 1.1 Students could carry out test-tube equilibrium shifts to show the effect of concentration and temperature (eg Cu(H₂O)₆²⁺ with concentrated HCl).$

Content

Opportunities for skills development

Many chemical reactions are reversible. In a reversible reaction at equilibrium: forward and reverse reactions proceed at equal rates the concentrations of reactants and products remain constant Le Chatelier’s principle. Le Chatelier's principle can be used to predict the effects of changes in temperature, pressure and concentration on the position of equilibrium in homogeneous reactions. A catalyst does not affect the position of equilibrium. Students should be able to: use Le Chatelier’s principle to predict qualitatively the effect of changes in temperature, pressure and concentration on the position of equilibrium explain why, for a reversible reaction used in an industrial process, a compromise temperature and pressure may be used.

PS 1.1 Students could carry out test-tube equilibrium shifts to show the effect of concentration and temperature (eg Cu(H₂O)₆²⁺ with concentrated HCl).