Hi guys,
I have a small question regarding reaction intermediates/writing the overall equation which I don't understand. Let's say I have the hypothetical equation shown below:
A+B<--> 2X (In equilibrium)
X-->C (Slow)
If I were to write the overall reaction of this reaction, my professor said I would write:
A+B-->2C Because my professor said the stoichiometric number of step two would be two so I would get rid of the intermediate.
I however wrote the overall equation to be:
A+B--> X+C I argued... if you form two molecules of a species in the first step, why can one of them not react with another species to form a product, while the other one stays as a product. My professor didn't explain himself at all and it made no sense why that couldn't happen.
I then told him, let's say I have the following mechanism:
A+B-->X
2X--->C
The first step in the mechanism would have to be done twice because my reactant is 2X in the second step, so I would have to form two products in step one so the overall equation would then be: 2A+2B-->C
I guess my question is, why can I not form two molecules of a species in my first step, then one of the those molecules act as an intermediate to form another product, and the other molecule stay as a product of the reaction like my proposed mechanism of:
A+B<--> 2X (In equilibrium)
X-->C (Slow)
With me saying the overall reaction is A+B-->X+C
Any help would be GREATLY appreciated! Thanks!