expresses the reactant concentrations as a function of time. aa products kinetics are first order...
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ln[A] = -kt + ln[A] 0 3.The integrated rate law for a first-order reaction also can be expressed in terms of a ratio of [A] and [A] 0 as follows:TRANSCRIPT
•Expresses the reactant concentrations as a function of time.
aA → products
•Kinetics are first order in [A], and the rate law isRate = k[A]
•Integrated first-order rate law isln[A] = -kt + ln[A]0
1.Equation shows how concentration of A depends on time. If the initial concentration of A and the rate constant k are known, the concentration of A can be calculated at any time.
ln[A] = -kt + ln[A]0
2. Equation is of the form y = mx + b, where a plot of y versus x is a straight line with slope m and intercept b.
y = ln[A] x = t m = -k b = ln[A]0
Thus, for a first-order reaction, plotting the natural logarithm of concentration vs. time always gives a straight line. For the reaction,
aA → productsthe reaction is first order in A if a plot of ln[A] vs. t is a straight line.
ln[A] = -kt + ln[A]0
3. The integrated rate law for a first-order reaction also can be expressed in terms of a ratio of [A] and [A]0 as follows:
kt
]A[]A[ln 0
2N2O5(g) → 4NO2(g) + O2(g)
Since the plot of ln[N2O5] vs. time is a straight line, it confirms that the reaction is first order in N2O5, since it follows the equation ln[N2O5] = -kt + ln[N2O5]0.
•Half-life = the time required for a reactant to reach half its original concentration.•Designated by the symbol t1/2.
•General equation for the half-life of a first order reaction is (derivation in textbook (p. 542):
•Note for a first-order reaction, the half-life does not depend on concentration.
kt 693.0
2/1
•General reaction:aA → products
•That is second order in A, the rate law is:Rate = k[A]2
•The integrated second-order rate law has the form
1.A plot of 1/[A] vs. t will produce a straight line with a slope equal to k.
0]A[1
]A[1 kt
0]A[1
]A[1 kt
02/1 ]A[
1k
t
•The rate law for a zero-order reaction is:Rate = k[A]0 = k(1) = k
•For a zero-order reaction, the rate is constant. •It does not change with concentration as it does for first-order or second-order reactions.
•Integrated rate law for a zero-order reaction is:[A] = -kt + [A]0 Plot of [A] vs. t gives a straight line.
Half-Life equation:
kt
2]A[ 0
2/1