Answer:
[tex]\large\boxed{\large\boxed{0.529M}}[/tex]
Explanation:
Since the rate constant has units of s⁻¹, you can tell that the order of the reaction is 1.
Hence, the rate law is:
[tex]r=d[A]/dt=-k[A][/tex]
Solving that differential equation yields to the well known equation for the rates of a first order chemical reaction:
[tex][A]=[A]_0e^{-kt}[/tex]
You know [A]₀, k, and t, thus you can calculate [A].
[tex][A]=0.548M\times e^{-3.6\cdot 10^{-4}/s\times99.2s}[/tex]
[tex][A]=0.529M[/tex]
The value of the concentration of A is 0.529.
Since the rate constant has units of s⁻¹, we can tell that the order of the reaction is 1.
[tex](A)=A_{0} e^{-kt}[/tex]
Here, [tex]A_{0}[/tex] is the initial concentration, t is the time, A is the final concentration, and k is the rate constant.
Substitute the given value values in the equation as follows,
[tex](A)=0.548M e^{-3.6*10^{-4s^{-1}\times99.2s } } \\=0.529M[/tex]
The concentration of A in (M) is 0.529.
Find more information about first- order reaction here,
brainly.com/question/13309369
