Description
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) | 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 |
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?
Explanation & Answer
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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.