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प्रश्न
From the following data, show that the decomposition of hydrogen peroxide is a reaction of the first order:
| t (min) | 0 | 10 | 20 |
| V (ml) | 46.1 | 29.8 | 19.3 |
Where t is the time in minutes and V is the volume of standard KMnO4 solution required for titrating the same volume of the reaction mixture.
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उत्तर
k = `2.303/"t" log (["A"_0])/(["A"])`
k = `(2.303/"t") log ("V"_0/"V"_"t")`
In the present case, V0 = 46.1 ml.
The value of k at each instant can be calculated as follows:
| t (min) | Vt | k = `(2.303/"t") log ("V"_0/"V"_"t")` |
| 10 | 29.8 | k = `2.303/10 log (46.1/29.8)` = 0.0436 min−1 |
| 20 | 19.3 | k = `2.303/20 log (46.1/19.3)` = 0.0435 min−1 |
Thus, the value of k comes out to be nearly constant. Hence it is a reaction of the first order.
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