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posted by  The King Cobra on 12/1/2008 12:28:14 AM  |  status: Live  

Will rate life saver. Plz need help

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Question Details:
Consider the following three-step mechanism:
(1) A(g) B(g) [fast]

(2) B(g) + 2C(g) D(g) [slow]

(3) D(g) E(g) [fast]
(a) Complete the balanced overall reaction below.
  • Enter any non-one coefficients in their own boxes.
  • Enter all species in alphabetical order.
+

(b) Which of the following species are intermediates? (Select all that apply.)











(c) What is the molecularity of each step? Enter your answers as numbers.
Step 1 =
Step 2 =
Step 3 =
(d) Complete the rate law for the overall reaction.
  • Enter your answers with square brackets to indicate concentration.
  • List all species in alphabetical order.
  • Use a '^' to indicate a non-one power. (Ex. [X][Y]2 should be entered [X][Y]^2.)
rate = k
Tags: Chemistry
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posted by Werner on 12/1/2008 4:16:10 AM  |  status: Live
Asker's Rating: Lifesaver   
The King Cobra's comment:
"thanks a lot"
Response Details:
                           A(g) B(g) [fast] 
 
                            B(g) + 2C(g) D(g) [slow] 
 
                            D(g) E(g) [fast]
 ---------------------------------------------------
  Over all reaction:  A(g) +  2C(g) ----------> E(g)
 -----------------------------------------------------
  b)   B(g) and D(g) are intermediates. Because they are obtained in one step and consumed in another step.
  c) the molecularity of each step
Step 1 =
Step 2 =
Step 3 =
 d) The rate law for the over all reaction
    A(g) +  2C(g) ----------> E(g)
    Rate = k[A][C]2
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