Data for the decomposition of hydrogen peroxide at some set temperature T is provided below. The rate law depends only on the concentration of H2O2. (These same data will be used for questions 6, 7 and 8.) 2 H2O2 ---> 2 H2O O2 t (seconds) 0 60 120 180 240 360 420 600 [H2O2] (M) 0.882 0.697 0.566 0.458 0.372 0.236 0.188 0.094 What is the value of the rate constant, k

is the value of the rate constant.

Explanation:

Let the order of the reaction be x.

The rate law of the reaction can be written as:

1. Rate of the reaction when concentration changes from 0.882 M to 0.697 M in 0 seconds  to 60 seconds.

..[1]

2. Rate of the reaction when concentration changes from  0.697 M to 0.566 M in 240 seconds to 360 seconds.

..[2]

[1] ÷ [2]

Solving fro x:

x = 0.92 ≈ 1

is the value of the rate constant.

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