Unit 6:Thermochemistry.
6.1 Endothermic and Exothermic Processes.
Determine if a process is endothermic or exothermic and assign the
proper sign to ∆H.
6.2 Energy Diagrams.
Identify reactants and products as being higher in energy on an energy
diagram.
Determine if a process is endothermic or exothermic from an energy
diagram.
Calculate ∆H from values on an energy diagram.
6.3 Heat Transfer and Thermal Equilibrium.
Interpret a particle diagram using arrows to show heat transfer.
Justify energy transfer as resulting from collisions between warmer and
cooler particles.
Assign the direction of heat flow based on temperature data for two
system components.
6.4 Heat Capacity and Calorimetry.
Calculate any variable in q = mc∆T for heating, cooling, and phase
changes.
Use conservation of energy to calculate temperature changes based on
heat lost/gained by another substance.
6.5 Energy of Phase Changes.
Differentiate between energy changes due to heating/cooling and phase
transitions in a pure substance.
Calculate the heat of a phase change given temperature, mass, and
enthalpy of phase change data.
6.6 Introduction to Enthalpy of Reaction.
Describe energy exchange between reaction systems and surroundings.
Calculate the amount of heat absorbed/released in a reaction using ∆H in
a stoichiometric calculation.
Compare and contrast the chemical potential energy of reactants and
products in a system.
6.7 Bond Enthalpies.
Justify the sign of ∆H by comparing bond strengths of reactants and
products.
Calculate ∆H using bond energies and the equation ∆H = ∑[bonds broken] -
∑[bonds formed].
6.8 Enthalpy of Formation.
Calculate ∆H using enthalpies of formation and the equation ∆H°rxn =
∑∆Hf°prod - ∑∆Hf°react.
6.9 Hess’s Law.
Identify a valid series of steps for an overall process, considering
stoichiometry and energy change.
Manipulate reaction steps to match an overall process and calculate ∆H.
Use Hess’s law results to justify the overall sign of a process, even if
component steps have different signs.