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 why conservation of atoms means a balanced equation predicts product amounts from reactant amounts, and reactant amounts from product amounts. (Guide: “Why a balanced equation lets you predict amounts”; Practice Q7)
- I can explain why coefficients are mole ratios and not mass ratios. (Guide: Worked example 1; Practice Q1)
- I can define the limiting reactant, the excess reactant, theoretical yield and percent yield. (Guide: “Limiting reactant, excess reactant and yield”)
Calculation
- I can follow the road map from a given quantity to moles, across the mole ratio, and on to the wanted quantity. (Guide: Figure 1; Worked example 1)
- I can use molarity to find moles from a solution volume, and the volume of solution needed for a reaction. (Practice Q4)
- I can use PV = nRT to turn moles of a gas into a volume, with T in kelvin. (Guide: Worked example 2; Practice Q5)
- I can identify the limiting reactant by comparing moles divided by coefficients. (Guide: Worked example 2; Practice Q2, Q6)
- I can calculate the theoretical yield, the excess left over and the percent yield. (Practice Q6)
- I can check an answer with conservation of mass or conservation of atoms. (Guide: Worked example 1; Practice Q7)
Reasoning
- I can predict how the amount of product changes when the amount of one reactant changes, and say whether that reactant is limiting or in excess. (Guide: Figure 2; Practice Q3, Q6(e))
- I can explain a limiting-reactant result at the particle level, describing what is left after the reaction. (Practice Q7)
- I can state the assumptions behind a stoichiometry calculation, such as completion and a single reaction. (Revision notes)
All ticked? Move on to Topic 4.6, Introduction to Titration, or return to the course roadmap.