General Chemistry II

What you'll learn

• Apply the first law of thermodynamics with correct sign conventions, calculate pressure–volume work, distinguish enthalpy from internal energy, and use calorimetry data from coffee-cup and bomb calorimeters to find heat capacities, enthalpies of reaction and fuel energies.
• Calculate enthalpy changes using Hess’s law, standard enthalpies of formation and average bond enthalpies, and use them to compare fuels, foods and enthalpies of solution.
• Predict and calculate entropy changes, apply the second and third laws, and use ΔG = ΔH − TΔS and free energies of formation to judge spontaneity and find crossover temperatures.
• Express concentrations as molality and mole fraction, and apply Henry’s law, Raoult’s law, boiling point elevation, freezing point depression and osmotic pressure, including van ’t Hoff factors, molar mass determination and reverse osmosis.
• Define and measure reaction rates, determine rate laws and rate constants by the method of initial rates and by integrated rate laws, and use half-lives to solve problems in pharmacology, radiocarbon dating and the environment.
• Explain rates with collision theory and energy profiles, use the Arrhenius equation to find activation energies and predict rates at other temperatures, evaluate reaction mechanisms against rate laws, and explain how catalysts and enzymes work.
• Write equilibrium constant expressions, relate K_c and K_p, use the reaction quotient to predict the direction of change, solve equilibrium problems with ICE tables, apply Le Châtelier’s principle, and connect K to ΔG° and temperature.
• Use solubility products to relate K_sp to molar solubility, predict precipitation, calculate the common-ion effect and the effect of pH on solubility, and design selective precipitations.
• Classify acids and bases by the Arrhenius, Brønsted–Lowry and Lewis definitions, calculate pH for strong and weak acids and bases, use K_a, K_b and K_w for conjugate pairs, predict the acidity of salt solutions, and relate acid strength to structure.
• Explain how buffers work, design buffers with the Henderson–Hasselbalch equation, calculate pH changes on adding acid or base, calculate titration curves for strong and weak acids, and choose suitable indicators.
• Balance redox equations by the half-reaction method, describe galvanic and electrolytic cells, calculate standard and non-standard cell potentials, relate E° to ΔG° and K, apply Faraday’s law, and explain batteries, fuel cells and corrosion protection.
• Combine thermodynamics, kinetics, equilibrium, solubility, acid–base chemistry and electrochemistry to analyze a real system, the carbon dioxide–carbonate chemistry of rain and seawater, and solve integrated multi-step problems.