The following reaction: CHCl3 (g) + Cl2 (g) --> CCl4 (g) + HCl (g) is believed t

Question

The following reaction: CHCl3 (g) + Cl2 (g) --> CCl4 (g) + HCl (g) is believed to process by this mechanism:

Step 1: Cl2 (g) <==> 2Cl (g)    (Fast) (Equilibrium State)

Step 2: Cl (g) + CHCl3 (g) --->  HCl (g) + CCl3 (g)      (Slow)

Step 3: CCl3 (g) + Cl (g) --->CCL4 (g)    (Fast)

The rate is determined to be Rate= k [Cl2]^1/2 [CHCL3].  Is the proposed mechanism consistent with the experimental rate law? Why or why not? (Work must be shown in determining the rate from the mechanism in the answer).

Explanation / Answer

here is the solved question for the same

http://books.google.co.in/books?id=2OxrDtDaSqIC&pg=PA743&lpg=PA743&dq=The+rate+is+determined+to+be+Rate%3D+k+[Cl2]^1/2+[CHCL3].+Is+the+proposed+mechanism+consistent+with+the+experimental+rate+law?&source=bl&ots=Br7OOopQSA&sig=FLPHZomG-aumnpwQR7OEu3dBd8o&hl=en&sa=X&ei=LfAFU7isLMyWrgflhoCAAQ&ved=0CC0Q6AEwAQ#v=onepage&q=The%20rate%20is%20determined%20to%20be%20Rate%3D%20k%20[Cl2]^1%2F2%20[CHCL3].%20Is%20the%20proposed%20mechanism%20consistent%20with%20the%20experimental%20rate%20law%3F&f=false

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