| Term | Definition |
|---|
| Law of Mass Action | The relationship between the concentration of reactants and products in a reaction at equilibrium is given by the equilibrium expression |
| Equilibrium | When the rate of forward reaction is equal to the rate of the reverse reaction |
| The Equilibrium Expression | Keq = ([C]^c [D]^d) / ([A]^a [B]^b) where aA + bB <--> cC + dD |
| Equilibrium Constant | Tells you the relative amounts of products and reactants at equilibrium |
| Keq and Gases | Kp = Kc (RT)^Δn |
| The Reaction Quotient | Q = ([C]^c [D]^d) / ([A]^a [B]^b) where aA + bB <--> cC + dD; Same as the equilibrium expression only that the initial conditions are used in place of equilibrium conditions |
| Keq and Multistep Processes | If A + B <--> C, Keq = K1; And C <--> D + E, Keq = K2; Then A + B <--> D + E, Keq = K1K2 |
| Haber Process | Used in the industrial preparation of ammonia (N2 + 3H2 <--> 2NH3) |
| Le Chatelier's Law | Whenever a stress is placed on a situation at equilibrium, the equilibrium will shift to relieve that stress |
| Concentration | When the concentration of a reactant or product is increased, the reaction will proceed in the direction that will use up the added substance (and vice versa) |
| Volume | When the volume in which a reaction takes place is increased, the reaction will proceed in the direction that produces more moles of gas (and vice versa) |
| Temperature | When temperature is increased, the reaction will proceed in the endothermic direction (and vice versa) |
Combine with other sets
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