A study of the rate of dimerization of C4H6 gave the data shown in the table: 2 C4H6 → C8H12 Time (s) 0 1600 3200 4800 6200 [C4H6 ] (M) 1.00 x 10-2 5.04 x 10-3 3.37 x 10-3 2.53 x 10-3 2.08 x 10-3 a) Determine the average rate of reaction between 0 s and 1600 s.
b) Determine the average rate of reaction between 1600 s and 3200 s. Using a spreadsheet program like Excel, plot [C4H6] vs time. Answer the following questions using graphical methods, i. e. draw tangent lines to curve by hand. Turn in the graph containing the tangent lines with the homework.
c) Estimate the instantaneous rate of reaction at 3200 s from a graph of time versus [C4H6]. What are the units of this rate?
d) Estimate of instantaneous rate of formation of C8H12 at 3200 s as well as the instantaneous rate of consumption of C4H6 at 3200 s. How do these rates compare to the rate of reaction at 3200 s?
e) Consider the reaction and the data given. Use a spreadsheet program like Excel and plot the integrated rate laws, [C4H6] vs. time, ln [C4H6] vs time, [C4H6] -1 vs time. Turn in ALL 3 of graphs with this problem.
f) Determine the order of the reaction with respect to C4H6.
g) Determine the value of the rate constant. (include units)
h) Write the rate law for this reaction.
i) What is the rate of reaction when [C4H6] = 3.00 x 10-3 M?
j) When the concentration of C4H6 is tripled, by what factor will the rate increase?