- #1
Foon
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I have no idea how to figure this one out, I've been hacking away at it all evening. Please help
Consider the general reaction:
2A + B --> 2E + F
The experimentally determined rate law equation is written as follows:
Rate = k[A]
A proposed mechanism for the reaction has the first step below:
Step 1: A + B --> C + F (rate determinging step)
Assuming a two-step mechanism, write a possible second elementary reaction for this mechanism.
And this is what I have but I'm not sure if its right. And I'm totally puzzled as to how they get rid of the C.
Step1: A + B --> C + F
Step2: A --> C- + 2E
------------------------
2A + B --> 2E + F
It has to be totally wrong since they've given me a rate law which I have no idea how to use.
Consider the general reaction:
2A + B --> 2E + F
The experimentally determined rate law equation is written as follows:
Rate = k[A]
A proposed mechanism for the reaction has the first step below:
Step 1: A + B --> C + F (rate determinging step)
Assuming a two-step mechanism, write a possible second elementary reaction for this mechanism.
And this is what I have but I'm not sure if its right. And I'm totally puzzled as to how they get rid of the C.
Step1: A + B --> C + F
Step2: A --> C- + 2E
------------------------
2A + B --> 2E + F
It has to be totally wrong since they've given me a rate law which I have no idea how to use.