CHEM 1001 Study Guide - Midterm Guide: Nitric Acid, Rate Equation, Amphoterism

• School: York University
• Department: Chemistry
• Course: CHEM 1001
• Professor: Donald Hastie

Document Summary

15. 1 dynamic equilibrium: 2 opposing processes taking place at equal rates: physical equilibrium situations: vapour pressure of liquid, solubility of solute, & distribution coefficient representing partitioning of solute between 2 immiscible solvents, chemical equilibrium: reactions being reversible. Note: change in n is from stoich. coefficients, not actual amounts. Also, equilibrium constant expressions don"t contain [solids] or [liquids] b/c their concentration stays constant cuz density. 15. 4 magnitude of an equilibrium constant: situations considered to not in equilibrium: reaction goes to completion if k > 1010 and basically doesn"t occur in forward direction if k < 10-10. 15. 5 reaction quotient q: predicting direction of net change: uses initial concentrations/activities w/ same form as equilibrium constant expression to predict direction. If q = k, reaction is at equilibrium. If q < k, then moves to right (forward reaction increases). If q > k, shifts left (reverse reaction increases). *note: equilibrium condition/constant doesn"t depend on reaction mechanism or catalysts.