For A yields products, time and concentration data were collected and plotted as
ID: 810221 • Letter: F
Question
For A yields products, time and concentration data were collected and plotted as shown here.
Table: [A](M) a. 0.750 , b. 0.596 , c. 0.473 , d. 0.376 ; t(s) a. 0.0 , b. 30.0 , c. 60.0 , d. 90.0
Plot [A]: exponential decrease; x-axis: t, y-axis: [A]
Plot ln[A]: constant decrease; x-axis: t, y-axis: ln[A]
Plot 1/[A]: exponential increase; x-axis: t, y-axis: 1/[A]
Determine the reaction order, the rate constant, and the units of the rate constant.
HINT: The integrated rate equations relate concentration, time, and the rate constant.
0th order: kt = [A]0 - [A]
1st order: kt = ln[A]0 - ln[A]
2nd order: kt = (1/[A]) - (1/[A]0)
Explanation / Answer
The order is going to be determined by the graph that has the straight line which is going to be the natural log graph, indicating that it is going to be first order. Since it is first order the units will be s-1 which can be seen by the slope (rise/run) which will be unitless/s (ln is unitless). To solve for the rate constant you will plug into the integrated rate law.
k(30s)=ln(0.750)-ln(0.596)
k=7.66*10-3s-1.
Hope this helps
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