Given the data below for the reaction, 2 A + 2 B + 4 C => D + E + 3 F, the react

Question

Given the data below for the reaction, 2 A + 2 B + 4 C => D + E + 3 F, the reaction is 1.----- order in A, 2.----- order in B, 3.----- order in C and 4.----- order overall. USE WORDS TO FILL IN THE BLANKS NOT NUMBERS (i.e., zero, first, second etc) !!!!! : Experiment Initial conc of A, mol/L Initial conc of B, mol/L Initial conc of C, mol/L Initial rate, mol/L.s 1 0.1 0.1 0.2 2 x 10-3 2 0.2 0.3 0.2 4 x 10-3 3 0.3 0.1 0.2 6 x 10-3 4 0.4 0.3 0.4 1.6 x 10-2

How do i figure this one out when one of the concentrations does not have a constant one so i can use it to compare with the otheres

Explanation / Answer

From experiments 1 and 3, we see that tripling the concentration of A has NO effect on the reaction rate. Thus, the reaction must be zeroth(!) order in A.

From experiments 2 and 3, we see that tripling the concentration of B results in tripling the rate (since we already know that the reaction is 0th order in A, we can ignore the change in A).

Finally, from experiments 2 and 4, we see that doubling the concentration of C results in doubling the reaction rate (again we can ignore the change in A), so the reaction is also 1st order in C.

Thus, in summary:

A: zeroth order
B: first order
C: first order

Overall: second order.

Note that the rate law does not have to related to the coefficients present in the balanced equation, and that some reagents may not even appear in the rate law!

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