1.  The rate of a reaction is influenced by


     A.  temperature.

     B.  the presence of a catalyst.

     C.  the activation energy for the reaction.

     D.  all of the above.


 2.  In the following reaction, the rate of appearance of CrO42-  is

     3.0 x 10-4 mol L-1 s-1.


     2 Cr3+(aq) + 3 IO4-(aq) + 10 OH-(aq) = 2 CrO42-(aq) + 3 IO3-(aq)

                                                       + 5 H2O(l)

     What is the rate of disappearance of IO4-?


     A.  2.0 x 10-4 mol L-1 s-1

     B.  3.0 x 10-4 mol L-1 s-1

     C.  4.5 x 10-4 mol L-1 s-1

     D.  6.0 x 10-4 mol L-1 s-1


 3.  If the rate expression for a reaction is:    Rate = k[NO][O3],

     the reaction is


     A.  first-order in O3.

     B.  second-order in NO.

     C.  third-order overall.

     D.  first-order overall.


 4.  If the rate law for a reaction is:     Rate = k[A][B],     what are

     the units of the rate constant?


     A.  (mol/L)3 s-1

     B.  (mol/L) s-1

     C.  (mol/L)-2 s-1

     D.  (mol/L)-1 s-1


 5.  For the reaction,	A(g)  =  B(g)  +  C(g), the following

     data on the initial rate of decomposition of A are collected.


	[A]o, M		Initial Rate, M/s

	0.10		      5

	0.30		     45


     Determine the order of the reaction in A and the rate constant

     of the reaction.


     A.  1,  k = 500 s-1

     B.  1,  k = 5 s-1

     C.  2,  k = 500 M-1 s-1

     D.  2,  k = 20 M-1 s-1


 6.  The rate of the reaction


2 HgCl2(aq)  +  C2O42-(aq)  =  2 Cl-(aq)  +  2 CO2(g)  +  Hg2Cl2(s)


     is followed by measuring the mass of Hg2Cl2 that precipitates.  From

     the following data for the reaction determine the rate law for the

     reaction.


	Expt	[HgCl2], M	[C2O42-], M	Initial Rate, M/min

	 1	  0.105	          0.15	          1.8 x 10-5

	 2	  0.105	          0.30	          7.2 x 10-5

	 3	  0.052	          0.30	          3.6 x 10-5

	 4	  0.052	          0.15	          8.9 x 10-6


     A.  Rate = k[HgCl2]2[C2O42-]

     B.  Rate = k[HgCl2][C2O42-]2

     C.  Rate = k[HgCl2]2

     D.  Rate = k[C2O42-]2


 7.  X + Y = Z is found to have the following rate law:  Rate = k[X]2[Y].

     What will be the effect on the initial rate if the concentration of

     both X and Y are doubled?


     A.  Rate increases by a factor of 4

     B.  Rate increases by a factor of 2

     C.  Rate increases by a factor of 8

     D.  Rate is unaffected


 8.  The decomposition of N2O5 in CCl4(l) at 45oC is found to follow

     first-order kinetics.  If the half-life for the reaction is 18.6

     min at 45oC, how long will it take 80.0 g of N2O5 to be reduced

     to 7.50 g at this temperature?


     A.  74.2 min

     B.  0.127 min

     C.  63.5 min

     D.  18.6 min


 9.  The reaction 2 AB2(g) = 2 A(g) + B2(g) has a rate constant

     k = 1.0 x 10-10 s-1 at 300 K and an activation energy of 111 kJ/mol.

     At what temperature will this reaction have a rate constant of

     k = 1.0 x 10-5 s-1?


     A.  238 K

     B.  405 K

     C.  187 K

     D.  1500 K


10.  Which of the following corresponds to the activation energy for the

     following exothermic reaction?




11.  For the reaction, NO2(g) + CO(g) = NO(g) + CO2(g), an

     acceptable mechanism is


NO2 + NO2 =  NO3 + NO     (slow)

NO3 + CO = NO2 + CO2       (fast)


     The corresponding rate law for this reaction must be


     A.  Rate = k[NO2]2

     B.  Rate = k[NO3][NO]

     C.  Rate = k[NO3][CO]

     D.  Rate = k[NO2][CO2]


12.  A catalyst is a substance that


     A.  increases the order of a reaction.

     B.  takes no part in a chemical reaction.

     C.  increases the rate of a reaction without being consumed.

     D.  increases the activation energy of a reaction.


13.  In which of the following is the oxidation state for the S atom

     incorrect?


     A.  H2SO3,  +4

     B.  S2O32-,  +3

     C.  H2S,  -2

     D.  Na2S2,  -1


14.  In which of the following is the oxidation state for the bolded

     atom incorrect?


     A.  HNO2,  +2

     B.  K2HPO4,   +5

     C.  KClO3,  +5

     D.  Ca(HCO3)2,   +4


15.  What are the stoichiometric coefficients for the following equation

     when it is properly balanced?


I2O5  +  CO  =   I2  +  CO2




             I2O5          CO           I2            CO2

     A.       5            1            1             5

     B.       5            1            5             1

     C.       1            5            5             5

     D.       1            5            1             5


16.  The anode in an electrochemical cell is always


     A.  the site where oxidation occurs.

     B.  connected to a salt bridge.

     C.  the electrode toward which cations migrate.

     D.  the electrode toward which electrons flow in the external circuit.


17.  In the following reaction of a galvanic cell


H2(g)  +  Cu2+(aq)  = 2 H+(aq)  +  Cu(s)


     A.  Cu2+(aq) is being oxidized.

     B.  H2(g) is the reducing agent.

     C.  H2(g) is being reduced.

     D.  Cu(s) is the anode.


18.  Given


Ca2+(aq)  +  2 e  =   Ca(s)          E  = -2.87 V

Cu2+(aq)  +  e   =   Cu+(aq)          E  = 0.16 V


     Find the standard potential for the reaction:


2 Cu2+(aq)  +  Ca(s)   =  Ca2+(aq)  +  2 Cu+(aq)


     A.  -3.03 V

     B.  +2.71 V

     C.  -2.71 V

     D.  +3.03 V


19.  For the galvanic cell


2 Ce4+(aq)  +  Co(s)   =   2 Ce3+(aq)  +  Co2+(aq)


     the potential, Ecello, is 1.89 V.  Given that the standard reduction

     potential, Eo, for the


Co2+(aq)  +  2 e  =   Co(s)


     half-reaction is -0.28 V, determine the standard reduction potential

     for

Ce4+(aq)  +  e   =   Ce3+(aq)


     A.  1.61 V

     B.  0.80 V

     C.  2.17 V

     D.  -2.17 V


20.  Use the following reduction potentials to identify a substance that

     will reduce Ag+(aq) to Ag(s) but not Ni2+(aq) to Ni(s).


			                Eo, V

          Mg2+(aq)  +  2 e   =   Mg(s)	-2.37

          Zn2+(aq)  +  2 e   =   Zn(s)	-0.76

          Ni2+(aq)  +  2 e   =   Ni(s)	-0.25

          Pb2+(aq)  +  2 e   =   Pb(s)	-0.13

          Ag+(aq)  +  e   =   Ag(s)	+0.80

          Br2(l)  +  2 e  =  2 Br-(aq)	+1.07


     A.  Mg2+

     B.  Br2

     C.  Zn

     D.  Pb


21.  In order for a reaction to be spontaneous


     A.  K  <  1

     B.  delta G  >  0

     C.  E  >  0

     D.  delta H  <  0


22.  Given

2 U3+(aq)  +  Cd2+(aq)  =  Cd(s)  +  2 U4+(aq)


     with Eo  = +0.207 V, what is the potential of this cell reaction at

     298 K when [U3+] = 1.00 x 10-3 M, [U4+] = 0.200 M, and [Cd2+] = 0.100 M?


     A.  +0.0415 V

     B.  -0.057 V

     C.  -0.124 V

     D.  +0.109 V


23.  Which of the following cannot be used for the cathodic protection

     of iron?


     A.  Zn

     B.  Sn

     C.  Mg

     D.  Al


24.  What are the electrode products when current is passed through an

     aqueous solution of KI?


     A.  K and O2

     B.  H2 and O2

     C.  K and I2

     D.  H2 and I2


25.  Calculate the mass of aluminum produced by passing 3.75 amperes of

     current through a molten mixture containing Al3+ for 3000 seconds.


     A.  0.117 g

     B.  1.05 g

     C.  3.16 g

     D.  9.44 g