1. Expresses the reactant concentrations as a function of time. aA → products Kinetics are first order in [A], and the rate law is Rate = k[A] Integrated first-order rate law is ln[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.

2. 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 = tm = -kb = 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 → products the reaction is first order in A if a plot of ln[A] vs. t is a straight line.

3. 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:

4. 2N 2 O 5 (g) → 4NO 2 (g) + O 2 (g) Since the plot of ln[N 2 O 5 ] vs. time is a straight line, it confirms that the reaction is first order in N 2 O 5, since it follows the equation ln[N 2 O 5 ] = -kt + ln[N 2 O 5 ] 0.

5. Half-life = the time required for a reactant to reach half its original concentration. Designated by the symbol t 1/2. 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.

6. 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.

7. 2.Equation shows how [A] depends on time and can be used to calculate [A] at any time t, provided k and [A] 0 are known. 2C 4 H 6 (g) →C 8 H 12 (g) – second-order since a plot of 1/[C 4 H 6 ] vs. t produces a straight line. Expression for the half-life of a second order reaction:

8. 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: