1.  Given the plot below calculate the average rate of the first-order

     reaction between t = 20 s and t = 40 s.




     A.  rate = 0.18 M/s

     B.  rate = 6 x 10-3 M/s

     C.  rate = 2.4 M/s

     D.  rate = 0.12 M/s


 2.  Consider the reaction     N2O4 ---> 2 NO2.    If [N2O4] = 0.060 M

     and [NO2] = 0 initially, what is [NO2] when [N2O4] = 0.020 M?


     A.  0.020 M

     B.  0.040 M

     C.  0.060 M

     D.  0.080 M


 3.  For the reaction NO  +  Cl2 ---> NOCl2 the rate expression has been

     determined to be:  rate = k[NO][Cl2]2.  What is the overall order

     of the reaction?


     A.  first

     B.  second

     C.  third

     D.  Need to know the reaction mechanism in order to make a

         determination.


 4.  Use the following experimental data to determine the rate law for

     the reaction      A +  B  --->  C.


     Experiment	 [A](M)     [B](M) 	Initial rate (M/s)

	1	  0.100	    0.100	4.0 x 10-5

	2	  0.100	    0.200	4.0 x 10-5

	3	  0.200	    0.100	16.0 x 10-5


     A.  rate = k[A][B]

     B.  rate = k[A]2

     C.  rate = k[A][B]0

     D.  rate = k[B]2


 5.  Determine the units for the rate constant for the reaction

     2 A  +  B ---> C, given the following experimental data:


     Experiment	 [A](M) 	 [B](M)     Initial rate (mol L-1 s-1)

         1	1.0 x 10-2	1.0 x 10-2	0.53 x 10-3

         2	2.0 x 10-2	1.0 x 10-2	1.06 x 10-3

         3	3.0 x 10-2	2.0 x 10-2	1.59 x 10-3

         4	2.0 x 10-2	2.0 x 10-2	1.06 x 10-3


     A.  s-1

     B.  L mol-1 s-1

     C.  mol L-1 s-1

     D.  The rate constant is dimensionless.


 6.  If the rate law for the reaction     A  +  2 B  --->  products

     is rate = k[A][B], what is the effect on the rate of tripling the

     concentration of A and doubling the concentration of B?


     A.  The rate increases by a factor of 4.

     B.  The rate increases by a factor of 1.5.

     C.  The rate increases by a factor of 5.

     D.  The rate increases by a factor of 6.


 7.  If a reaction is first-order with a rate constant of 5.48 x 10-2 s-1,

     how long will it take for 75% of the initial reactant to be consumed?


     A.  25.3 s

     B.  48.6 s

     C.  5.2 s

     D.  36.5 s


 8.  Calculate the activation energy of a first-order reaction if the

     rate constant at 400 K is 4.9 x 10-4 s-1 and the rate constant

     at 500 K is 0.18 s-1.


     A.  98 kJ

     B.  -55 kJ

     C.  4.7 x 103 kJ

     D.  1.3 x 102 kJ


 9.  The activation energy for a reaction can be determined from the

     slope of the curve that comes from a plot of


     A.  ln A vs. 1/T

     B.  k vs. T

     C.  A vs. T

     D.  ln k vs. 1/T


10.  Consider the following mechanism (all species are gases):


               Cl2 ---> 2 Cl		slow

               Cl  +  CO --->  COCl	fast

               COCl  +  Cl --->  COCl2	fast


     Which one of the following statements is false?


     A.  The overall reaction is Cl2 + CO ---> COCl2.

     B.  Cl is a catalyst.

     C.  COCl is an intermediate.

     D.  The rate law should be rate = k[Cl2].


11.  Which one of the following statements is true?


     A.	Exothermic reactions are always fast.

     B.	The rate law can be determined from the stoichiometry of the

        reaction.

     C.	The rate constant nearly always increases with temperature.

     D.	Catalysts increase the rate of the reaction and the value of the

        equilibrium constant.


12.  Which of the following statement(s) is/are true for a reaction where

     rate = k[A]?


          1.  The reaction is zero order.

          2.  A plot of ln[A] vs. time (or, t) gives a straight line.

          3.  t1/2 = 0.693 / k.

          4.  A plot of [A]-1 vs. time gives a straight line.


     A.  1

     B.  1 and 4

     C.  2

     D.  2 and 3


13.  In which one of the following is the oxidation state of the bolded

     atom given incorrectly?


     A.  ClO3-,  +5

     B.  NH3,  -3

     C.  Na2O2,  -2

     D.  S2O32-,  +2


14.  When the following reaction is balanced in acid solution, what is

     the ratio of MnO4- to Fe2+?


MnO4- +  Fe2+ ---> Mn2+  +  Fe3+


     A.  1 MnO4- :  2 Fe2+

     B.  1 MnO4- :  5 Fe2+

     C.  2 MnO4- :  3 Fe2+

     D.  2 MnO4- :  5 Fe2+


15.  Which one of the following statements is true in regard to a

     spontaneous redox reaction?


     A.  Ecello is always positive.

     B.  delta Go is always positive.

     C.  Eredo is always negative.

     D.  Eoxo is always positive.


16.  Which one of the following is the strongest oxidizing agent?


     A.  K+

     B.  K

     C.  Br2

     D.  Br-


17.  The voltage produced in the reaction


Fe(s)  +  Cu2+(aq)  ---> Cu(s)  +  Fe2+(aq)


     is independent of


     A.  the concentration of Cu2+.

     B.  the metal used as the anode.

     C.  the temperature.

     D.  the size of the cathode.


18.  Determine Eo for the reaction


2 Fe3+(aq) + Pb(s) ---> 2 Fe2+(aq) + Pb2+(aq)


     A.  0.90 V

     B.  0.64 V

     C.  1.03 V

     D.  0.51 V


19.  Which one of the following will reduce I2 under standard conditions

     but will not reduce H+?


     A.  O2

     B.  Cu

     C.  Ag

     D.  Zn2+


20.  If an electrochemical cell is based on the following reaction, what

     value of n should be used in the Nernst equation?


2 Al(s) + 3 Co2+(aq) ---> 2 Al3+(aq) + 3 Co(s)


     A.  2

     B.  3

     C.  6

     D.  5


21.  Determine the value of Keq at 25oC for the reaction


Cl2(g) + 2 Br (aq) ---> 2 Cl (aq) + Br2(l)


     A.  2.3 x 1041

     B.  8.1 x 104

     C.  6.5 x 109

     D.  1.5 x 10-10


22.  Calculate E for the voltaic cell


2 Ag+(aq)  +  Sn(s) ---> 2 Ag(s)  +  Sn2+(aq)


     at 298 K, if [Ag+] = 1.7 M and [Sn2+] = 0.15 M given:   Eo = +0.65


     A.  +0.65 V

     B.  +0.61 V

     C.  -0.65 V

     D.  +0.69 V


23.  Inhibiting the corrosion of a metallic object by placing it in

     electrical contact with a second, more reactive, metal is termed


     A.  electrorefining.

     B.  cathodic protection.

     C.  electromotive force.

     D.  electroplating.


24.  Molten MgCl2 is electrolyzed using inert electrodes.  Which one of

     the following statements is true?


     A.  Cl- is the oxidizing agent.

     B.  Oxidation occurs at the cathode.

     C.  The cations in the electrolyte undergo reduction.

     D.  The cathode experiences a loss of mass.


25.  How much Al(s) can be produced from Al3+ in 1.00 hr with a current

     of 1.00 amp?  (The molar mass of Al is 27.0 g/mol).


     A.  0.34 g

     B.  1.01 g

     C.  5.06 g

     D.  12.8 g