The experimentally determine rate law for the reaction AB + C rightarrow A + BC

Question

The experimentally determine rate law for the reaction AB + C rightarrow A + BC is: rate = K[AB]^2 Which statement is true regarding the proposed mechanism: AB + AB rightarrow AB_2 + A AB_2 + C rightarrow AB + BC Step 1 is the slow step. Step 2 is the slow step. Both steps have the same rate. The relative rates of the two steps cannot be determined. This mechanism cannot be correlated to The overall reaction. Kinetic data is collected, and In k.v.1/T is graphed for reactions 1 and 2. Which statement is true given the equation for the two graphs? Reaction 1:y =-22337x + 25.215 Reaction 2: y =-12459x + 31.603

Explanation / Answer

11)
step 1 should be the sloe step
since rate depends on the slowest step and step 1 is slow step
rate law will be
rate = k [AB]^2
which matches with the given rate law

Answer: A

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