Consider the proposed mechanism for the reaction, CHCl3(g) + Cl2(g) --> HCl(g) + CCl4(g) (1 - fast) Cl2(g) = 2 Cl(g)(2 - slow) Cl(g) + CHCl3(g) --> HCl(g) + CCl3(g)(3 - fast) Cl(g) + CCl3(g) --> CCl4(g) A student proposes that the reaction rate law is rate = k [Cl] [CHCl3]. Why is this incorrect? (Choose the best answer.) Group of answer choices The student's proposed rate law is not based on the rate-determining step in the mechanism. The rate orders with respect to Cl and CHCl3 match the stoichiometric coefficients for these compounds in step (2). It is always the last step in a mechanism that determines the rate law and CHCl3 is not in step (3). Cl is in the proposed rate law. Cl is an intermediate and only reactants and products that appear in the overall reaction equation may be in the reaction rate law.
Consider the proposed mechanism for the reaction, CHCl3(g) + Cl2(g) --> HCl(g) + CCl4(g)
(1 - fast) Cl2(g) = 2 Cl(g)
(2 - slow) Cl(g) + CHCl3(g) --> HCl(g) + CCl3(g)
(3 - fast) Cl(g) + CCl3(g) --> CCl4(g)
A student proposes that the reaction rate law is rate = k [Cl] [CHCl3]. Why is this incorrect? (Choose the best answer.)
The student's proposed rate law is not based on the rate-determining step in the mechanism.
The rate orders with respect to Cl and CHCl3 match the stoichiometric coefficients for these compounds in step (2).
It is always the last step in a mechanism that determines the rate law and CHCl3 is not in step (3).
Cl is in the proposed rate law. Cl is an intermediate and only reactants and products that appear in the overall reaction equation may be in the reaction rate law.
Trending now
This is a popular solution!
Step by step
Solved in 4 steps with 2 images