In a study of the gas phase decomposition of hydrogen peroxide at 400 degree C H

Question

In a study of the gas phase decomposition of hydrogen peroxide at 400 degree C H_2O_2(g) rightarrow H_2O(g) + 1/2 O_2(g). The following data were obtained: The observed half life for this reaction when the starting concentration is 0.104 M is s and when the starting concentration is 5.20 times 10^-2 M is The average delta(l/[H_2O_2])/delta t from t = 0 s to t =18.0 s is M^-1 s^-1. The average delta (I/[H_2O_2])/delta t from t = 18.0 s to t = 54.1 s is M^-1s^-1. Based on these data, the rate constant for this order reaction is M^-1s^-1

Explanation / Answer

Q1.

HL = time required for concentration to be halved

so

C1 = 0.104 --- > HL = 0.104/2 = 0.052,

from the table, this time is T = 18 seconds

and when

Cinitia = 5.2*10^-2, then -->

T = (54.1-18) = 36.1 seconds

Q2.

vg rate = Cfinal - Cinitial / (Tfinal - Tiniail)

the avg. rate of H2O2 --> (5.2*10^-2 - 0.104)/(18-0) = -0.00288888 M/s

the avg. rate of H2O2 --> (2.6*10^-2 - 5.2*10^-2 )/(54.1-18) = -0.000720M/s

Q3

this is clerly SECOND order, since it varies swith respect to time

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