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Consider the reaction: 3A + 2B ---> 2C + D Run [A] [B] Rate (M/ms) 1...

Consider the reaction:
3A + 2B ---> 2C + D

Run [A] [B] Rate (M/ms)
1 100 100 6.00E+3
2 200 300 144.00E+3
3 100 200 12E+3


Determine the rate expression and overall order for the above reaction.

Order with respect to B, given that A is constant should be 1 as doubling the concentration of B (runs 1 and 3) results in a doubling of the rate.

Order with respect to A should be 2 as the reaction rate is dependent on the concentration of both A and B (you cannot keep B constant and compare trials and rates).

Therefore the overall equation should be rate=k[A]^2 [A]^1

Thus, the overall order is 3. Is this correct?

Also, I notice that the rate in 2 is squared of the rate in 3. Can this also be used to determine?

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