AP Chemistry Full Mock Test 7
AP Chemistry Full Mock 7 focuses on thermodynamics and electrochemistry — Gibbs free energy, cell potential, Nernst equation, and electrolysis FRQs.
Emphasis: Thermodynamics and Electrochemistry
Full Mock 7 places significant question weight on Unit 9 — Gibbs free energy, entropy, cell potential, and the Nernst equation. These topics appear in nearly every AP Chemistry exam in some combination, and Mock 7 provides the concentrated full-exam practice needed to master them under realistic timed conditions.
Thermodynamics: What to Expect
Gibbs Free Energy Calculations
FRQ components in Mock 7 require calculating delta-G using delta-G equals delta-H minus T times delta-S, interpreting the sign of delta-G at different temperatures, and connecting delta-G to the spontaneity of the reaction. Temperature-dependent spontaneity (predicting the crossover temperature where spontaneity changes) is a frequent AP question type.
Entropy Reasoning
Mock 7 includes questions asking you to predict the sign of delta-S for reactions based on changes in phase, number of moles of gas, or molecular complexity. Justify entropy predictions at the molecular level — AP graders expect you to reference dispersal of energy or particles rather than just stating 'entropy increases.'
Electrochemistry: What to Expect
Standard Cell Potential FRQs
You will be asked to write half-reactions, identify cathode and anode, calculate E-cell from standard reduction potentials, and determine whether the reaction is spontaneous. Know the relationship between E-cell, delta-G, and K — AP FRQs frequently ask you to move between all three.
Nernst Equation Applications
Mock 7 includes Nernst equation problems under non-standard concentration conditions. Common FRQ structures: calculate E-cell at a given temperature and concentration, explain how cell voltage changes as the reaction proceeds, and determine the concentration of an ion from a measured cell potential.
Electrolysis Questions
Several MCQ and at least one FRQ component address electrolytic cells — predicting the product at each electrode, calculating the mass of metal deposited, and determining the time or current required for a given amount of electrolysis using Faraday's constant.