Hi. Happy almost Easter:) I need help with an overall order of a rate law questi

Question

Hi. Happy almost Easter:) I need help with an overall order of a rate law question. Molecule A is a first order reaction, Molecule B is a second order reaction and Molecule C is a zero order reaction. when all 3 are doubled, what happens to the rate of the reaction. I would think the rate would increase by 6 (the first order reaction would be doubled and the second order reaction would be quadrupled while the zero order would have no effect on the overall rate. 4 plus 2 is 6. 6 is not the correct answer, neither is 7 (if adding 1 for the zero order reaction).

Explanation / Answer

answer is 8 not 6 or 7

The rate law equation is ,

rate = k x (A)1 x (B)2

the above equation is first order wrt to A and seconf order wrt B and zero order as there is no C

Now double the conc of A and B

rate = k x (2A)1 x (2B)2

= 8 x (k x (A)1 x (B)2 )

= 8 x initial rate

So rate increases by 8 times

I am helpful i think

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