The decomposition of hydrogen peroxide was studied, and the following data were obtained at a particular temperature. time (s) [h2o2] (mol/l)0 1.00120 ± 1 0.91300 ± 1 0.78600 ± 1 0.591200 ± 1 0.371800 ± 1 0.222400 ± 1 0.133000 ± 1 0.0823600 ± 1 0.050 assuming that the rate= -delta [h2o2]/delta tdetermine the rate law, integrated rate law, and the value of the rate constant. calculate [h2o2] at 4000. s after the start of the reaction

answer; i do believe the correct answer is (river); /// good luck

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

the answer is 75.0%.