Predict equilibrium shifts with K, Q, and Le Chatelier’s principle without mixing up position, rate, or direction
4 sections · 8 lessons
Define reversible reactions, dynamic equilibrium, and equilibrium constants, then separate K from reaction rate and read what K values mean.
2 lessonsCompare Q with K, build ICE tables for equilibrium amounts, and predict how concentration changes move a system by tracking Q.
3 lessonsTrace how pressure, volume, and temperature changes alter gas equilibria, including the role of Δn(gas) and the temperature dependence of K.
2 lessonsDistinguish equilibrium position from time to equilibrium and repair the most common errors with clear checks.
1 lessonEvery lesson in order.
8 lessons
Chemical equilibrium begins when reversible reactions keep running in both directions while the amounts of reactants and products stop changing overall. This course builds the core tools for reading that state, from equilibrium constants and reaction quotients to shifts caused by concentration, pressure, volume, temperature, and catalysts. It is designed for beginner college chemistry students who need a clear, quantitative way to reason about equilibrium instead of memorizing slogans. By the end, the balance between forward and reverse change is much easier to track on paper and in problems.
This course covers dynamic equilibrium, K expressions, and the meaning of K magnitude, along with reaction quotient Q and Q versus K direction tests. It also includes ICE-table setup, concentration stresses, gas pressure and volume effects, temperature-driven shifts for endothermic and exothermic reactions, catalysts, and common misconception repair.
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