For a reaction of the form, A + B + C Products, the following observations are m

Question

For a reaction of the form, A + B + C Products, the following observations are made: doubling the concentration of A increases the rate by a factor of 4, doubling the concentration of B has no effect on the rate, and doubling the concentration of C increases the rate by a factor of 4. Write down the rate law for this reaction.

By what factor will the rate of the reaction described above change if the concentrations of A, B, and C are all halved (reduced by a factor of 2)?

I am well aware that the answer is D but my question how do you determine the answer? Please be very specific with the exponents because other wise i will not under stand. And once the exponents are there is there a certain way the multiply it and divide it?


a) The rate will change by a factor of 0.25.
b) The rate will change by a factor of 0.5.
c) The rate will change by a factor of 0.03125.
d) The rate will change by a factor of 0.0625.
e) The rate will change by a factor of 1.

Explanation / Answer

Rate = [A]^2[B]^0[C]^2 If all concentrations are halved Then Rate = [A]^2[B]^0[C]^2/16 d) The rate will change by a factor of 0.0625.

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