Question

In: Chemistry

1. You perform some experiments for the reaction A→B+C

The rate law has the form: rate = k[A]x . Calculate the value of x for each of the following:

[A] is tripled, but there is no effect on the rate.

[A] is tripled, and the rate increases by a factor of 27.

2. FOR THE REATCION 2NO2→ 2NO(g) + O2 (g) the data given below was collected.

Time(s) 0s 1.0s 2.0s 3.0s

[NO2] 0.1103 0.1076 0.1050 0.1026

Obtain the average rate of decomposition of NO2 in units of M/s for each interval.

What is the order of the reaction with respect to NO2?

How long would it take for the concentration to decrease to 0.0900 M?

Solutions

Expert Solution

1. You perform some experiments for the reaction A→B+C

The rate law has the form: rate = k[A]x . Calculate the value of x for each of the following:

[A] is tripled, but there is no effect on the rate.

Since rate is not affected by changing [A], it is zero order reaction. So

[A] is tripled, and the rate increases by a factor of 27.

But

Hence,

Thus, the reaction is of third order in A.

2. The average rate of decomposition of NO2

With decrease in the concentration of NO2, the rate of the reaction decreases. This is characteristic of first order reaction.

Let t be the time required to decrease the concentration to 0.0900 M. The average rate of decomposition of NO2 will be slightly less than 0.0024 M/s but for simplicity, we assume it to be 0.0024 M/s

Hence, it will take 8.3 s for the concentration to decrease to 0.0900 M.

queen_honey_blossom answered 1 year ago

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