Answer:
2.038 seconds.
Explanation:
So, in the question above we are given the following parameters in order to solve this question. We are given a rate constant of 0.500 s^-, initial concentration= 0.860 M and final concentration= 0.310 M,the time,t =??.
Assuming that the equation for the first order of reaction is given below,that is;
A ---------------------------------> products.
Recall the formula below;
B= B° e^-kt.
Therefore, e^-kt = B/B°.
-kt = ln B/B°.
kt= ln B°/B.
Where B° and B are the amount of the initial concentration and the amount of the concentration remaining, k is the rate constant and t = time taken for the concentration to decrease.
So, we have; time taken,t = ln( 0.860/.310)/0.500.
==> ln 2.77/0.500.
==> time taken,t =2.038 seconds.
The time taken should be 2.038 seconds.
Here we used the first order of reaction:
Since
B= B° e^-kt.
So, e^-kt = B/B°.
-kt = ln B/B°.
kt= ln B°/B.
Where B° refers initial concentration
And, B refers amount of the concentration remaining,
k is the rate constant
and t = time taken for the concentration to decrease.
Now
t = ln( 0.860/.310)/0.500.
ln 2.77/0.500.
,t =2.038 seconds.
Learn more about concentration here:https://brainly.com/question/4438044
