Assessment Objectives

Detailed Breakdown: Thermodynamics

• Define standard enthalpy of combustion ($\Delta H^\theta_c$), formation ($\Delta H^\theta_f$), and average bond enthalpy.
• Define entropy ($S$) and Gibbs free energy ($G$).
• Construct a Hess cycle to calculate an unknown enthalpy change from enthalpies of formation or combustion.
• Calculate the enthalpy of reaction using average bond enthalpies ($\Delta H = \Sigma \text{Bonds Broken} - \Sigma \text{Bonds Formed}$).
• Solve experimental problems using $q = mc\Delta T$ to find enthalpy changes per mole.
• Predict the spontaneity of a reaction using $\Delta G = \Delta H - T\Delta S$.
• Compare experimental calorimetry results to literature values and identify sources of error (e.g. heat capacity of the calorimeter).
• Discuss the temperature dependence of $\Delta G$ and its impact on reaction spontaneity.
• Analyze entropy changes for phase changes and chemical reactions and relate them to disorder.