Answer: The rate constant for the given reaction is [tex]4.33\times 10^{-6}s^{-1}[/tex]
Explanation:
For the given chemical equation:
[tex]CH_3NC(g)\rightarrow CH_3CN(g)[/tex]
We are given that the above equation is undergoing first order kinetics.
The equation used to calculate rate constant from given half life for first order kinetics:
[tex]t_{1/2}=\frac{0.693}{k}[/tex]
The rate constant is independent of the initial concentration for first order kinetics.
We are given:
[tex]t_{1/2}[/tex] = half life of the reaction = [tex]1.60\times 10^5s[/tex]
Putting values in above equation, we get:
[tex]k=\frac{0.693}{1.60\times 10^5s}=4.33\times 10^{-6}s^{-1}[/tex]
Hence, the rate constant for the given reaction is [tex]4.33\times 10^{-6}s^{-1}[/tex]
The rate constant when the initial [CH3NC] is 0.030 M will be equal to [tex]4.33*10^-^6s^-^1[/tex]
The equation is: [tex]k= \frac{0.693}{T_\frac{1}{2} }[/tex]
In this case, the symbol [tex]T_\frac{1}{2}[/tex] refers to the half-life value that we have in the above question.
[tex]k=\frac{0.693}{1.60*10^-^6s} = 4.33*10^-^6s^-^1[/tex]
More information about half-life in the link:
https://brainly.com/question/11152793
