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31 Dec 2017

77. Consider this three-step mechanism for a reaction: Cl2(8) 201(8) Fast Cl(8) + CHCl3(8) + HCl(9) + CC13(8) Slow CI(g) + CC13(8) T CC14(8) Fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. What is the predicted rate law?

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Related questions

The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine: 1) Cl2 â 2 Cl (fast, reversible) 2) Cl + CHCl3 â HCl + CCl3 (slow) 3) Cl + CCl3 â CCl4 (fast) What rate law does this mechanism predict? Choose from the list below and enter the letters for all the terms needed in the rate law. (So for a rate law of k[Cl2] enter AC, and for a rate law of k[Cl2][CHCl3] enter ACE.)

A. k G. [CCl3]1/2 M. [Cl2]2 B. [HCl] H. [HCl]1/2 N. [Cl]2 C. [Cl2] I. [Cl2]1/2 O. [CHCl3]2 D. [Cl] J. [Cl]1/2 P. [CCl3]2 E. [CHCl3] K. [CHCl3]1/2 F. [CCl3] L. [HCl]2

A proposed reaction mechanism is shown below:

A + B ^â_â 2 C (Fast)

2 C + D â E (Slow)

E + F â D + G + H (Fast)

a) Write the overall reaction represented by this mechanism. ,b) Identify any intermediates and any catalysts in this mechanism. c) Determine the rate law predicted by this mechanism. ddetermine the rate law predicted by this mechanism..e,What would you need to do to know whether this mechanism is potentially valid?.

Three part rate law question:) Will always thumbs up if the answer is right. Thanks again!

Part a)

Consider the overall reaction: AB(g) + CB(g) â¶ A(g) + CB2(g)

A proposed mechanism for this reaction is

2 AB(g) â AB2(g) + A(g) (fast)

AB2(g) + CB(g) â¶ AB(g) + CB2(g) (slow)

Based on this mechanism, determine the rate law for the overall reaction.

Part b)

Consider the following three-step mechanism for a reaction:

Br2 (g) â 2 Br (g) Fast

Br (g) + CHBr3 (g) â HBr (g) + CBr3 (g) Slow

Br (g) + CBr3 (g) â CBr4 (g) Fast

Based on this mechanism, determine the rate law for the overall reaction.

Part c)

Phosgene (Cl2CO), a poison gas used in World War I, is formed by the reaction of Cl2 and CO. The proposed mechanism for the reaction is
Cl2 â 2 Cl (fast,equilibrium)
Cl + CO â ClCO (fast,equilibrium)
ClCO + Cl2 â Cl2CO + Cl (slow)

Based on this mechanism, determine the rate law for the overall reaction.

Express your answers in terms of k and the necessary concentrations (ex: k[X][Y]^2). Use brackets around the concentrations and the caret symbol prior to the exponent. Do not include any multiplication signs.