Consider the reaction: 3a + b + 2 c -> d + e where rate = k[a]2 [c]2 .a reaction was performed where [b]o = [c]o = 0.600 m and [a]o = 2.20 x 10-5 m. a plot of 1/[a] vs time (min) gave a plot with a straight line relationship and after 7.00 min, [a] = 2.4 x 10-6 m. what was the initial rate of the reaction described above?

Explanation:

As the given reaction is

Also,  rate = k

So, rate is zero order with respect to B and it is second order with respect to both A and C.

It is given that [A] = and

For second order rate law, equation is as follows.

                    k =

As, the initial rate = k

                              = 0.412 \times 10^{5} M^{-1} sec^{-1} \times (2.20 \times 10^{-5} M)^{2} \times (0.6 M)^{2}" alt="2.20 \times 10^{-5} M" />

For second order rate law, equation is as follows.

                    k =

As, the initial rate = k

                              = 0.412 \times 10^{5} M^{-1} sec^{-1} \times (2.20 \times 10^{-5} M)^{2} \times (0.6 M)^{2}" />

                               =

Thus, we can conclude that the initial rate of the reaction described above is .

explanation: no but i do not usually comment

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