Ap Chemistry Equilibrium Flashcards

5638787709	Equilibrium constant	k=products-reactants	0
5638787710	K>1	Forward reaction is favored	1
5638787711	Forward reaction	Reactants to Products	2
5638787712	Reverse reaction	Products to reactants	3
5638787713	K<1	Reverse reaction is favored	4
5638787714	K=1	neither reaction is favored	5
5638787715	Small equilibrium constant means...	reactants are favored	6
5638787716	Large equilibrium constant means...	products are favored	7
5638787717	Kc and Kp have what units?	they both have no units, but Kp is calculated using atm and Kc is calculated using molarity	8
5638787718	1 atm	760 mmHg and 760 Torr	9
5638787719	What equation connects Kp and Kc?	Kp = Kc(RT)deltaN [delta N= (c+d) - (a+b)]	10
5638787720	Solids and liquids are...	completely omitted from calculations	11
5638787721	Reaction Quotient	measures the progress of a reaction relative to equilibrium	12
5638787722	How is q calculated?	Same way as Kc	13
5638787723	Difference between K and Q	Q depends on what STATE of the reaction and K has a given temperature that has only one value that specifies a relative amount	14
5638787724	If the reaction only contains reactants...	Q = 0	15
5638787725	If the reaction only contains products...	Q = infinity	16
5638787726	At equilibrium....	K = Q	17
5638787727	Q > K	reactions goes to the left (reactants)	18
5638787728	Q < K	reaction goes to the right (products)	19
5638787729	Q = K	reaction is at equilibrium	20
5638787730	Solubility product constant (Ksp)	Measures solubility of a compound	21
5638787731	Molar solubility	Solubility of a compound in. moles per liter	22
5638787732	Gibbs free energy equation with K	Grxn = -RT lnK At equilibrium G = 0	23
5638787733	When K<1 and Q=1	lnK is negative, G is positive, the reaction is spontaneous in the reverse direction	24
5638787734	When K>1 and Q=1	lnK is positive, G is negative, the reaction is spontaneous in the forward direction	25
5638787735	Le Chateller's Principle	when a chemical system at equilibrium is disturbed, the system shifts in the direction that minimizes the disturbance	26
5638787736	Adding product...	shifts left	27
5638787737	Adding reactant...	shifts right	28
5638787738	Removing product...	shifts right	29
5638787739	Removing reactant...	shifts left	30
5638787740	Increasing volume...	decrease in pressure and shifts toward the side with the more moles	31
5638787741	Decreasing volume...	increase in pressure and shifts toward the side with the least amount of moles	32
5638787742	In an endothermic reaction, increasing temperature means...	adding reactant, shifts right, and the value of K increases because the concentration of the products increase and the concentration of the reactants decrease.	33
5638787743	In an endothermic reaction, decreasing temperature means...	removing reactant, shifts left, value of K decreases because the concentration of the products decrease and the concentration of the reactants increase.	34
5638787744	In an exothermic reaction, increasing temperature means...	adding product, shifts left, value of K decreases because concentration of the products decrease and the concentration of the reactants increase.	35
5638787745	In a exothermic reaction, decreasing temperature means...	removing product, shifts right, value of K increases because the concentration of the products increase and the concentration of the reactants decrease.	36
5638787746	Adding a catalyst...	DOES NOT change the concentration	37
5638787747	Adding an inert gas...	DOES NOT change the concentration	38
5638787748	If the reaction is reversed	invert Kc	39
5638787749	If the reaction is multiplied	raise Kc to the power	40
5638787750	If the reaction is added	multiply Kc	41