Chemistry Kinetics Problem!

Chemistry
Tutor: None Selected Time limit: 1 Day

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. 

2 H2O2   --->   2 H2O  + O2

t (seconds)060120180240360420600
[H2O2] (M)0.8820.6970.5660.4580.3720.2360.1880.094

 1) What is the value of the rate constant, k?

2) What is the half life of the reaction when the initial concentration of H2O2  is 0.882 M?

3) What is the average rate of reaction, R,  from t = 60 to t = 120?

Sep 27th, 2015

Thank you for the opportunity to help you with your question!

The given reaction is first order reaction because in equal time interval equal proportion of rectant reacted.

1. So we have K= ln({Ao]/[A])/t=putting [Ao]=0.822 and

 [A]=.697 and t=20 we get k=3.923*10^-3 or 

alternatively = k[H2O2] 0.882-0.697/60 = k *0.882 k = 0.00349 s^-1

2. Half life, t/2= ln2/K=176.8 s

3. Average rate= change in concentration /time taken=0.697-0.566/60 = 2.18333m0l/s.

Please let me know if you need any clarification. I'm always happy to answer your questions.
Sep 27th, 2015

For number 1 choices are only: (a) 3.7x10^-3 /s, (b) 0.12 /s, (c)270 /s, (d) -3.7x10^-3, (e) 0.12 M/s

Sep 27th, 2015

For number 2 my choices are only: (a) 120 s, (b) 5.8 s, (c) 0.0053 s, (d) 155 s, (e) 190 s

Sep 27th, 2015

For number 3 my choices are only: (a) 0.13 M, (b) 0.065 M/s, (c)0.0011 M/s, (d) 910 M/s, (e) 0.0022 M/s

Sep 27th, 2015

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