Consider this overall reaction, which is experimentally observed to be second order in AB and zero order in C.
AB + C ---> A + BC
Is the following mechanism valid for this reaction? Why or why not?
AB + AB ----> AB2 + A (slow)
AB2 + C ----> AB + BC (fast)
Consider this overall reaction, which is experimentally observed to be second order in AB and zero order in C.
AB + C ---> A + BC
the following mechanism is valid for this reaction
AB + AB ----> AB2 + A (slow)
AB2 + C ----> AB + BC (fast)
because
we know that the rate determining step is the slowest step in the mechanism.
therefore
for the reaction step
AB + AB ----> AB2 + A (slow)
we have
rate = k [AB]^2
and this the rate of the slowest step and therefore rate of the reaction is
rate = k [AB]^2
therefore
we can say that the given mechanism is valid because the mecahnism shows that the reaction is second order in AB and zero order in C.
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