Kinetics (AP) Flashcards

7970304317	differential rate laws	reveal the relationship between the concentration of reactants and the rate of the reaction	0
7970304318	integrated rate laws	reveals the relationship between concentration of reactants and time	1
7970304319	reaction rate	the change in concentration of a reactant or product per unit of time	2
7970304320	differential rate law equation	rate=k[A]^m[B]^n	3
7970304321	rate of appearance	change in [product] ---------------------------------- change in time (t2-t1)	4
7970304322	rate of disappearance	change in [reactant] -------------------------------------- change in time(t2-t1) the rate at which one species disappears	5
7970304323	Determination of reaction order	Experimentally from the data	6
7970304324	zeroth order reactions	doubling the concentration has no effect on the rate at which this reaction occurs	7
7970304325	first order reaction	doubling the concentration of that species doubles the rate of the reaction	8
7970304326	second order reaction	doubling the concentration of that species quadruples the reaction rate; half-life doubles	9
7970304327	how to find the overall rate of the reaction	determine the sum of the exponents in the rate law	10
7970304328	factors affecting reaction rate	-surface area -concentration of reactants -temperature -nature of reactants (ie. solutions, gases) -catalysts (absence or presence of)	11
7970304330	activated complex	the (temporary) structure created at the point of maximum energy along the reaction path; aka transition state	12
7970304331	exothermic reaction	the potential energy of the REACTANTS is greater than that of the products	13
7970304332	endothermic reaction	the potential energy of the PRODUCTS is greater than that of the reactants	14
7970304333	activation energy	minimum energy required to start a reaction; energy at which successful collisions can occur	15
7970304336	delta E	the energy lost or gained in a reaction (through work or heat or both)	16
7970304337	kinetic control	thermodynamically favored processes that don't occur at measurable rates because of the high amount of activation energy needed for the reaction to take place	17
7970304338	thermodynamically favoured	spontaneous	18
7970304339	arrhenius equation	k=A^-Ea/RT	19
7970304340	R	ideal gas constant	20
7970304341	reaction mechanisms	the series of steps that sum to the overall reaction allows successful collisions to take place	21
7970304342	unimolecular reactions	reactions that happen in one step	22
7970304343	reaction intermediate	a substance that is produced and then consumed during the overall reaction	23
7970304344	rate determining step	the slowest elementary step in a reaction	24
7970304345	method of determining the rate law	Only through experimentation	25
7970304347	termolecular reactions	these reactions are very rare and they require the simultaneous collision of 3 particles with sufficient energy and the correct orientation	26
7970304348	catalyst	lowers the activation energy of a reaction; doesn't appear in the overall reaction	27
7970304349	acid-base catalysis	the catalyst of the reaction is an acid or a base	28
7970304350	surface catalysis	increases the number of collisions that have the correct orientation	29
7970304351	enzyme	biological catalyst	30
7970304353	units for k in a zero order reaction	M/s	31
7970304354	units for k in a first order reaction	1/s	32
7970304355	units for k in a second order reaction	1/Ms	33
7970304356	units for k in a third order reaction	1/M^2ᐧs	34
7970304357	first order integrated rate law	ln[A]=-kt + ln[A]o	35
7970304358	first order reaction graphs	plotting ln[A]t vs. time for first order reactions produce a straight line with a negative slope	36
7970304359	half-life	the time it takes for the concentration of a reactant to decrease by half	37
7970304360	half-life eqn (first order)	ln 2/k	38
7970304362	2nd order integrated rate law	1/[A]=kt + 1/[A]o	39
7970304363	graph for second order reactions	when plotting 1/[A]t vs. time, a straight line with a positive slope is produced	40
7970304364	What is the only factor that can affect the activation energy of a reaction?	the addition of a catalyst	41
7970304365	4 ways to speed up a reaction	increase temperature increase surface area increase concentration add a catalyst	42
7970304367	homogeneous catalyst	a substance that is consumed in one step of the reaction mechanism but is a product in a subsequent step	43
7970304368	heterogeneous catalyst	a catalyst that exists in a difference phase from that of reactants and products	44
7970304369	graph of zero order	plotting concentration vs. time producing a straight line and a negative slope	45
7971079243	spontaneous reaction	thermodynamically favourable rxn (delta G is a negative value)	46
7973160921	molecularity	number of molecules that participate as reactants in an elementary reaction	47
7973163331	bimolecular reaction	reaction that involves the collision of two molecules	48
7973198567	adsorption	binding of molecules to a surface (usually the first step in heterogeneous catalysis	49
7973221135	multistep mechanism	consists of a sequence of elementary steps	50
7973233746	decreases	reaction rate ___________ as Ea increases	51
7973748077	method of initial rates	allows for determination of k, and order of reactants	52
7973752394	order of a reactant	the exponent to which the [reactant] must be raised in the differential rate law	53