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Chapter 15: Equilibrium, 15.6: Disturbing a Chemical Equilibrium, 15.1:…
Chapter 15: Equilibrium
Equilibrium: when a chemical reaction moves forwards and backwards at the same rate (reactants convert to products and products convert to reactants simultaneously) 
Equilibria are dynamic means that changing the concentration of one (product or reactant) requires changing the others to restore equilibrium
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The reaction quotient, Q, uses the same formula as K and can show whether a reaction is at equilibrium or not
When Q = K, the reaction is at equilibrium
When Q < K, the direction of the reaction is reactants --> products (fowards)
When Q > K, the direction fo the reaction is reactants <-- products (backwards)
When using Q, the values for the concentration do not need to be at equilibrium
ICE tables show the initial concentration, change in concentration and the concentration at equilibrium for a reaction ICE Table Examples[/Equilibria/Le_Chateliers_Principle/Ice_Tables]
When stoichiometric coefficients of a balanced equation are multiplied by some factor, the equilibrium constant for the new equation is the old equation constant raised to the power of the multiplication factor
1: (rxn), Kc
2: x(rxn) , Kc^x
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When two or more chemical equations are added to produce a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants for the added equations
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15.2: Understand Kc and Kp. Predict whether a reaction is reactant or product favored at equilibrium based on K value. Find Q and relate it to K.
15.3: Calculate an equilibrium constant given reactant and product concentrations at equilibrium. Calculate an equilibrium constant given the initial concentrations and one of the equilibrium concentrations
15.5: Know how K changes as different stoichiometric coefficients are used in a balanced equation, if the equation is reversed or if several equations are added to give a new net equation
Changing temperature, concentrations or volume will have an effect on the equilibrium