Work through the list without notes. If you cannot do a statement, follow its link, then come back. Guide = study guide; Practice = practice questions.
Understanding
- I can explain how experimental data show that a system has reached equilibrium. (Guide: Figure 1; Practice Q5(e))
- I can explain why only equilibrium values, not starting values, go into K. (Guide: “Common misconceptions”; Practice Q3)
- I can explain why experiments at the same temperature give the same K even when their concentrations differ. (Practice Q7(b))
Calculation
- I can calculate Kc from a set of equilibrium concentrations. (Guide: Worked example 1(a); Practice Q1)
- I can calculate Kp from equilibrium partial pressures, leaving out any solid. (Guide: Worked example 1(b); Practice Q2)
- I can convert moles to mol L⁻¹ before using Kc. (Guide: Worked example 2)
- I can build an ICE table from starting amounts and one measured equilibrium value, using the coefficients for the change row. (Guide: Worked example 2; Practice Q3, Q5)
- I can allow for dilution when two solutions are mixed. (Practice Q5(b))
- I can turn a total pressure into partial pressures using the mole ratio of the gases. (Guide: Worked example 3; Practice Q6)
- I can use a known K to find one missing equilibrium concentration. (Practice Q7(c))
Reasoning
- I can explain, using the powers in the expression, how one equilibrium concentration must change when another changes at constant K. (Guide: “Reading K as a relationship”; Practice Q4)
- I can spot a calculation error when two experiments at the same temperature give very different K values. (Guide: “Reading K as a relationship”; Practice Q7)
All ticked? Move on to Topic 7.5, Magnitude of the Equilibrium Constant, or return to the course roadmap.