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Enter your answer in the provided box. The first-order reaction of decomposition of azomethane is given below: CH3―N═N―CH3(g) → N2(g) + C2H6(g) At a certain temperature, the rate constant for this reaction equals 2.35 × 10−3 s−1. Calculate the half-life of this reaction (in seconds) at the same temperature.

Respuesta :

Answer:53,5seconds

Explanation:

The half- life of the given reaction is 294.9 s.

Relationship between half life and rate constant for first order

[tex]t_{1/2} =\frac{0.6932}{k}[/tex]

Here, [tex]t_{1/2}[/tex] is the half life, and k is the rate constant.

We can calculate the half- life from the above reaction as follows,

[tex]t_{1/2}=\frac{0.6932}{2.35 \times10^{-3} s^{-1} } =0.294\times10^{3}s\\=294.9 s[/tex]

So, the half- life for the decomposition of azomethane is 294.9s.

Find more information about half-life here,

brainly.com/question/24710827

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