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 say what the sign of ΔH tells me about heat released or absorbed at constant pressure. (Guide: “What the enthalpy of reaction tells you”; Practice Q1)
- I can explain that ΔH refers to one mole of reaction, for the amounts and states in the equation as written. (Guide; Practice Q1)
- I can explain how a change in chemical potential energy becomes a change in the kinetic energy of particles, and so a temperature change. (Guide: “Where the energy comes from”; Practice Q4)
- I can describe how the products reach thermal equilibrium with the surroundings in exothermic and endothermic reactions. (Guide: Figure 1; Practice Q6)
Calculation
- I can calculate q from the mass or moles of any reactant or product, dividing by its coefficient. (Guide: Worked examples 1 and 2; Practice Q2)
- I can work backwards from a required amount of energy to the mass of reactant needed. (Guide: Worked example 1; Practice Q7)
- I can scale and reverse a thermochemical equation and give the new ΔH. (Guide: “Scaling and reversing”; Practice Q3)
- I can use the limiting reactant to find the moles of reaction and the heat transferred. (Guide: Worked example 3; Practice Q5)
- I can find ΔH from calorimetry data using q_rxn = −q_soln. (Practice Q6)
Reasoning
- I can evaluate a claim about how changing the amount of one reactant changes the heat released. (Practice Q5)
- I can explain why breaking bonds needs energy and forming bonds releases it, and link this to the sign of ΔH. (Guide: “Common misconceptions”; Practice Q7)
All ticked? Move on to Topic 6.7, Bond Enthalpies, or return to the course roadmap.