REACTION MECHANISM MULTIPLE CHOICE TEST

Read carefully the questions:
1.  The number of molecules that participate as reactants in an elementary step is the _______ of the step.
          a.  elementary step
          b.  molecularity
          c.  multistep mechanism
          d.  reaction mechanism
2.  It is formed in one elementary step and is consumed in the next step.
          a.  molecularity
          b.  intermediate
          c.  catalyst
          d.  elementary step
3.  Which step of the reaction is the rate-determining step?
          a. the fastest step
          b. the last step in the reaction mechanism
          c.  the first step
          d.  the slow step
4. When a lit match is touched to the wick of a candle, the candle begins to burn.  When the match is removed, the candle continues to burn; the match
          a.  behaves as a catalyst.
          b.  supplies the activation energy.
          c.  is part of the rate-determining step.
          d.  lowers the activation energy barrier.
5. A catalyst increases the rate of a reaction by
          a.  increasing the concentration of the reactants(s).
          b.  decreasing the concentration of the reactant(s).
          c.  increasing the activation energy of the overall reaction.
          d.  decreasing the activation energy of the overall reaction.
6.  Consider the following mechanism:  Step 1:  Cl  +   O₃  →  ClO  +  O₂
                                                           Step 2:  O +  ClO  → Cl  +  O₂
     The reaction intermediate is
          a.  Cl
          b.  O₂
          c.  O₃
          d.  ClO
For questions 7-9, refer to this problem:  Consider  the reaction of H₂ and HCl as shown in the mechanism below:
             H₂(g)  +  ICl(g)  → HI(g)    +   HCl(g)
             HI(g)   +  ICl(g)   →   I₂(g)   +  HCl(g)
7.  What is the overall reaction of the reaction above?
          a.  H₂(g)  +  ICl(g)  +  HI(g)  →   I₂(g)   +   2HCl(g)
          b.  H₂(g)  +  2ICl(g)   →   I₂(g)  +  2HCl(g)
          c.  HI(g)   +   ICl(g)   →   2HCl(g)
          d.  H₂(g)   +   HI(g)   →  I₂(g)   +   ICl(g)
8.  What is the intermediate?
          a.  H₂
          b.  HI
          c.  ICl
          d.  HCl
9.  What is the overall rate law if the first step is slow and the second step is fast?
          a.  Rate = k[H₂][ICl]
          b.  Rate = k[HI][ICl]
          c.  Rate = k[H₂][ICl]²
          d.   Rate = k[H₂][HCl]
10.  Which equation below is an example of bimolecular reaction?
          a.  O₃(g)  →   O₂(g)  +  O(g)
          b.  2NOBr(g)  +   Br₂(g)  →   2NOBr(g)
          c.  2H₂O₂(aq)   →   2H₂O(l)   +   O₂(g)
          d.  2SO₂(g)   +   O₂(g)  →   2SO₃(g)

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