In a study of the gas phase decomposition of hydrogen peroxide at 400 °C the fol

Question

In a study of the gas phase decomposition of hydrogen peroxide at 400 °C the following data were obtained: 5.80x10-2 25.3 2.90x10-2 59.0 H202l. M 0.232 0.116 seconds 8.43 Hint: It is not necessary to graph these data. The observed half life for this reaction when the starting concentration is 0.232 M is concentration is 0.116 M is s and when the starting The average (1 [H202]) . At from t = 0 s to t = 8.43 s is The average (11H,O2]) . At from t = 8.43 s to t = 25.3 s is M S Based on these data, the rate constant for this order reaction is M S

Explanation / Answer

Q1

the time stated --> Tfinal - tinitial = 8.43-0 = 8.43 seconds

for 2nd:

the time stated --> Tfinal - tinitial = 25.3-8.43 = 16.87 seconds

Q2

Rate = (0.116-0.232)/8.43 = -0.01376

Rate = ((5.8*10^-2) - 0.116 )/16.87 = -0.00343

Q3

this must be 2nd order, since halfl life depends on initial conditions

so

k = 1/([A0]*t)

k = 1/(0.232*8.43) = 0.5113 1/(M-s)

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