If the net reaction A+B yields C proceeds by a single-step bimolecular mechanism, is it true that this must be a second order equation since it proceeds in only a single-step mechanism?
The Question taken out of the next was:
For the net reaction A+B yields C, which proceeds by a single-step bimolecular mechanism, which one of the following equations hold true?
a) t1/2 = 0.693/k
b) Rate of reaction = k[A]
c) Rate of appearence of C = rate of disappearence of A
d) ln [A] = -kt +ln[A]0
My guess is that a and d are both incorrect, because the reaction is at least a second order reaction. The answer in my book says c, but why would b be incorrect? Additionally is there a difference between rate of appearence and rate of formation. In a similar question, the rate of formation of a product was said to equal the negative rate of disappearence of the reactant. In order to make since, wouldn't answer c have to be worded rate of appearence of C = -rate of disappearenc of A?
If anybody can help, thank you