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Answer:
The average reaction rate between 0 and 1500 s?rate [tex]=1.12*10^{-4} M/s[/tex]. The average reaction rate between 200 and 1200 s ? rate [tex]=1.10*10^{-4} M/s[/tex]. The instantaneous rate of the reaction at t=800 s?rate [tex]=7.1*10^{-5} M/s[/tex].
Explanation:
The average rate of a chemical reaction is a function of the change in the concentration of reactants or products and the time taken for the change to happen. The instantaneous rate is estimated by considering the average rate at the smallest possible time interval such as Δt tends to zero.
1) The average reaction rate between 0 and 1500 s?
rate = (0.184-0.016)M/(1500-0)s [tex]=1.12*10^{-4} M/s[/tex].
2) The average reaction rate between 200 and 1200 s ?
rate = (0.129-0.019)M/(1200-200)s [tex]=1.10*10^{-4} M/s[/tex].
3) The instantaneous rate of the reaction at t=800 s?
In this case, we consider the data directly before and after the given point. Such as (0.069 M, 500 s) and (0.019 M,1200 s)
instantaneous rate = (0.069 - 0.019)M/(1200-500)s [tex]=7.1*10^{-5} M/s[/tex].
We ignore the negative sign because we are only interested in the magnitude of the reaction rate.
The average rate for given reactions is [tex]1.12 \times 10^{-4} {\rm \ M/s}[/tex] and [tex]1.10 \times 10^{-4} {\rm \ M/s}[/tex].
What is the average rate?
It is the time rate of change in the concentration of reactants or products in the given time.
So, the average rate between 0 -1500 s:
[tex]R_{avg} = \dfrac {(0.184-0.016) {\rm \ M}}{(1500-0){\rm \ s} }\\\\R_{avg} = 1.12 \times 10^{-4} {\rm \ M/s}[/tex]
The average rate between 200 and 1200 s :
[tex]R_{avg} = \dfrac {(0.129-0.019) {\rm \ M}}{(1200-200){\rm \ s} }\\\\R_{avg} = 1.10 \times 10^{-4} {\rm \ M/s}[/tex]
Therefore, the average rate for given reactions is [tex]1.12 \times 10^{-4} {\rm \ M/s}[/tex] and [tex]1.10 \times 10^{-4} {\rm \ M/s}[/tex].
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