This collection of classroom resources features activities from our Equilibria course for teachers, from our Teaching Chemistry series. This collection is most valuable to those who have attended this course and wish to put into practice with their students some of the ideas and activities presented as part of that event. Please note that this list is not exhaustive; not all trainer activities have a corresponding classroom resource. In some circumstances there is variation between the training resource and classroom resource.
This programme is designed to develop students understanding through basic concepts such as reversible and irreversible reaction, looking at both physical and chemical changes, to dynamic equilibria and factors that affect equilibria. Working through the activities will also develop thinking and research skills.
This activity demonstrates the links between the topics of rates of reaction and the equilibrium law. It provides students with an explanation of the equilibrium law and helps them explain why Le Chatelier’s principle works for temperature, concentration and pressure.
Assessment for Learning is an effective way of actively involving students in their learning. Each session plan comes with suggestions about how to organise activities and worksheets that may be used with students.
Using iodine crystals dissolved in equal volumes of two immiscible solvents, students can create an equilibrium distribution.
Use your microscale titration apparatus to determine the equilibrium constant for the reaction between silver(I) and iron(II) ions
The reversible reaction between bismuth(III) oxychloride and bismuth(III) chloride is demonstrated in this experiment.
Changing the chlorine concentration or temperature in this reaction shifts the position of equilibrium, demonstrating Le Chatelier’s principle.
Watch as the equilibrium between cobalt species Co(H2O)62+ and CoCl42- is disturbed – with an accompanying colour change predicted by Le Chatelier’s principle.
Turn a mixture of methyl red indicator and soda water from red to yellow, and create a less acidic solution as the equilibria adjusts.
Explore the effect of pressure and temperature on the equilibrium between nitrogen dioxide and dinitrogen tetroxide.
This activity shows the students the fundamental link between entropy and equilibrium and increases students’ understanding of scientific models. It highlights the importance of mathematical descriptions in physical chemistry.