Ap Chemistry Equilibrium Flashcards

11852767526	Equilibrium constant	k=products-reactants	0
11852767527	K>1	Forward reaction is favored	1
11852767528	Forward reaction	Reactants to Products	2
11852767529	Reverse reaction	Products to reactants	3
11852767530	K<1	Reverse reaction is favored	4
11852767531	K=1	neither reaction is favored	5
11852767532	Small equilibrium constant means...	reactants are favored	6
11852767533	Large equilibrium constant means...	products are favored	7
11852767534	Kc and Kp have what units?	they both have no units, but Kp is calculated using atm and Kc is calculated using molarity	8
11852767535	1 atm	760 mmHg and 760 Torr	9
11852767536	What equation connects Kp and Kc?	Kp = Kc(RT)deltaN [delta N= (c+d) - (a+b)]	10
11852767537	Solids and liquids are...	completely omitted from calculations	11
11852767538	Reaction Quotient	measures the progress of a reaction relative to equilibrium	12
11852767539	How is q calculated?	Same way as Kc	13
11852767540	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
11852767541	If the reaction only contains reactants...	Q = 0	15
11852767542	If the reaction only contains products...	Q = infinity	16
11852767543	At equilibrium....	K = Q	17
11852767544	Q > K	reactions goes to the left (reactants)	18
11852767545	Q < K	reaction goes to the right (products)	19
11852767546	Q = K	reaction is at equilibrium	20
11852767547	Solubility product constant (Ksp)	Measures solubility of a compound	21
11852767548	Molar solubility	Solubility of a compound in. moles per liter	22
11852767549	Gibbs free energy equation with K	Grxn = -RT lnK At equilibrium G = 0	23
11852767550	When K<1 and Q=1	lnK is negative, G is positive, the reaction is spontaneous in the reverse direction	24
11852767551	When K>1 and Q=1	lnK is positive, G is negative, the reaction is spontaneous in the forward direction	25
11852767552	Le Chateller's Principle	when a chemical system at equilibrium is disturbed, the system shifts in the direction that minimizes the disturbance	26
11852767553	Adding product...	shifts left	27
11852767554	Adding reactant...	shifts right	28
11852767555	Removing product...	shifts right	29
11852767556	Removing reactant...	shifts left	30
11852767557	Increasing volume...	decrease in pressure and shifts toward the side with the more moles	31
11852767558	Decreasing volume...	increase in pressure and shifts toward the side with the least amount of moles	32
11852767559	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
11852767560	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
11852767561	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
11852767562	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
11852767563	Adding a catalyst...	DOES NOT change the concentration	37
11852767564	Adding an inert gas...	DOES NOT change the concentration	38
11852767565	If the reaction is reversed	invert Kc	39
11852767566	If the reaction is multiplied	raise Kc to the power	40
11852767567	If the reaction is added	multiply Kc	41