Determination of order by initial rates For each experiment, examine the first p
ID: 537414 • Letter: D
Question
Determination of order by initial rates For each experiment, examine the first plot from part B of the report, the plot of A_infinity - A_t. Select the points at the beginning of the plot which form a straight line: that is when the change in absorbance appears to be most linear. Remember that there will be a "lag" phase in the plot, where the concentration values change very little, which should be ignored In other words, you should skip the first point(s) of the plot which do not contribute to the straight-line portion. Be sure to refer back to the discussion about Figure 8 on page 57. Plot the data points you selected using Excel and use the trendline option to find the equation of the straight line and the value of R^2. The slope of the line will represent the rate of the reaction. Put these values in the table on the bottom of this page. Attach both plots to your report. Be sure to appropriately title! Calculate the initial concentration of Cr^3+ for both experiments. First, report the actual volumes you used for each experiment in the table below. Then, show your work for experiment 1 in the space below, and report the values in the table at the bottom of the page. Determine the order of the reaction with respect to Cr^3+ using the values you placed in the table at the bottom of this page. Show your work in the space below.Explanation / Answer
12) Make use of the dilution law:
M1*V1 = M2*V2 where M1 = concentration of the original solution; M2 = concentration of dilute solution; V1 = volume of the original solution and V2 = volume of dilute solution.
Experiment 1:
Plug in the values: M1 = 0.100 M; V1 = 1.00 mL; V2 = 31.00 mL.
Therefore,
(1.00 mL)*(0.100 M) = (31.00 mL)*M2
===> M2 = (1.00*0.100 M)/(31.00) = 0.0032258 M 0.00323 M
The concentration of CrCl3 in the dilute solution is 0.00323 M (ans).
Experiment 2:
Plug in the values: M1 = 0.100 M; V1 = 2.00 mL; V2 = 31.00 mL.
Therefore,
(2.00 mL)*(0.100 M) = (31.00 mL)*M2
===> M2 = (2.00*0.100 M)/(31.00) = 0.0064516 M 0.00645 M
The concentration of CrCl3 in the dilute solution is 0.00645 M (ans).
13) I need the value of the rate to answer the question.
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