The Concept of Equilibrium, The Equilibrium Constant, Understanding and Working with Equilibrium Constants, Heterogenous Equilibria, Calculating Equilibrium Constants, Applications of Equilibrium Constants, Le Chatelier's Principle
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| 331814727 | chemical equilibrium | the rate at which the products form from the reactants equals the rate at which the reactants for the products (opposing reactions proceeding at equal rates) | |
| 331814728 | Haber process | the catalyst system and conditions of temperature and pressure developed by Fritz Haber and coworkers for the formation of NH₃ (ammonia) from H₂ and N₂ Real- Life Application: The quantity of food required to feed the ever increasing human population far exceeds that provided by nitrogen- fixing plants. Therefore, human agriculture requires substantial amounts of ammonia- based fertilizers for croplands. | |
| 331814729 | la of mass action | the relationship between the concentrations of the reactants and products present at equilibrium general equilibrium equation: aA +bB ↔ dD +eE where A, B, D, E are chemical species involved and a, b, d, and e are their coefficients | |
| 331814730 | equilibrium-constant expression | see bk pg 614 | |
| 331814731 | equilibrium constant (kc) | the numerical value obtained when we substitute molar equilibrium concentrations into the equilibrium- constant expression | |
| 331814732 | homogenous equilibria | equilibria involve substances that are all in the sam phase (usually gas or liquid) | |
| 331814733 | heterogenous equilibria | substances in equilibria are in different phases | |
| 331814734 | reaction quotient (Q) | a number obtained by substituting reactant and product concentrations or partial pressures at any point during a reaction into an equilibria-constant expression | |
| 331814735 | Comparing Q and K | The possible situations:
Q=K: the reaction quotient equals the equilibrium constant only if the system is at equilibrium
Q>K: the concentration of products is too large and that of reactants too small. Substances on the right side of the chemical equation react to form substances on the left; the reaction proceeds from right to left to approach equilibrium
Q| | |
| 331814736 | Le Châtelier's principle | a principle stating that when we disturb a system at chemical equilibrium, the relative concentrations of reactants and products shift so as to partially undo the effects of the disturbance |
