Homework Answers
Answer:
The plot [R] vs time is shown below
![0.006 (Os, 0.006M) 0.005 |(15s, 0.00478M) On [R] (mol/L) (100s, 0.00136) (125s, 0.000957) 0.001 0.000- 0 50 100 200 250 300 1](http://img.homeworklib.com/questions/77681290-3167-11eb-b230-6bce04a73484.png?x-oss-process=image/resize,w_560)
(Since 1 mol/L=1M)
Rate = ΔC/ Δt=|C2-C1|/(t2-t1)
Rate (t=0s to t=15s)=|Ct=15s - Ct=0s|/(15s-0s)=|(0.00478 M - 0.006 M)|/(15s)
Rate (t=0s to t=15s)=8.133 x 10-5 M/s
Rate (t=100s to t=125s)=|Ct=125s - Ct=100s|/(125s-100s)=|(0.000957 M - 0.00136 M)|/(25s)
Rate (t=100s to t=125s)=1.612 x 10-5 M/s.
Please let me know if you have any doubts. Thanks.
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concentration of the reactant. In the case of second-order
reactions, the rate is proportional to the square of the
concentration of the reactant.
Select the image to explore the simulation, which will help you
to understand how second-order reactions are identified by the
nature of their plots. You can also observe the rate law for
different reactions.
In the simulation, you can select one of the three different...
The half-life of a reaction,
t1/2, is the time it takes for the reactant concentration [A] to
decrease by half. For example, after one half-life the
concentration falls from the initial concentration [A]0 to [A]0/2,
after a second half-life to [A]0/4, after a third half-life to
[A]0/8, and so on. on. For a first-order reaction, the half-life is
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