Chemical Equilibrium Review
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| 15.1) What is the point at which the concentrations of all species are constant? | Chemical equilibrium
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| 15.1) In a rate law, are the concentrations of just reactants, just products, or both included? | Reactants
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| 15.1) What type of equilibrium exists when the rates of the forward and reverse reactions are equal? | Dynamic
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| 15.2) What is K subscript c? | The equilibrium constant in terms of concentration
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| 15.2) What is K subscript p? | The equilibrium constant in terms of pressure
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| 15.2) In an equilibrium-constant expression, is K subscript c equal to the concentration of reactants over the the concentration of products? | No, concentration of products over concentration of reactants
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| 15.2) Which phases of matter are eliminated from equilibrium-constant expressions? | Solids and liquids
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| 15.2) In the general expression relating K subscript c and K subscript p, how is the change in n calculated? | Moles of gaseous product - moles of gaseous reactant
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| 15.3) If K >> 1, do products or reactants dominate at equilibrium? | Products
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| 15.3) If K << 1, do products or reactants dominate at equilibrium? | Reactants
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| 15.3) How is the equilibrium constant for the forward reaction related to the equilibrium constant for the reverse reaction? | Reciprocals
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| 15.3) How is the equilibrium constant for a net reaction of two or more steps determined? | Product of K's for individual steps
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| 15.4) What type of equilibria has all reactants and products present in the same phase? | Homogeneous
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| 15.4) What type of equilibria has products and reactants present in different phases? | Heterogeneous
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| 15.6) What is used to determine the value of the equilibrium expression, when the system is not at equilibrium? | Q, the reaction quotient
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| 15.6) How are Q and K related when the system is at equilibrium? | Q = K
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| 15.6) How are Q and K related when the forward reaction must occur to reach equilibrium? | Q < K
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| 15.6) How are Q and K related when the reverse reaction must occur to reach equilibrium? | Q > K
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| 15.7) What is the term for a system that will shift its equilibrium position to counteract the effects of a disturbance? | Le Chatelier's Principle
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| 15.7) What disturbances does Le Chatelier's Principle include? | Change in: temperature, pressure, concentration
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| 15.7) If you remove product from a system at equilibrium, which way does the reaction proceed? | Toward the product
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| 15.7) If the pressure is increased in a gaseous system, which way does the reaction proceed? | Toward the direction with fewer moles
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| 15.7) What happens to K when increasing the temperature of an endothermic reaction? | Increases
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| 15.7) What happens to K when increasing the temperature of an exothermic reaction? | Decreases
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| 15.7) How does a catalyst speed up a reaction? | Lowers activation energy
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