The following data was collected for the concentration of a reactant as a function of time. Use MS Excel to determine what the order of the reaction is and the rate constant. Attach graphs to report.
Time (sec) | Concentration [M]
0 | 1
100 | 0.96
200 | 0.92
500 | 0.82
750 | 0.75
1000 | 0.69
2000 | 0.53
3000 | 0.43
5000 | 0.31
Rxn Order =
9. Variation of the rate constant with temperature for the first-order reaction below is given in the following table
2 N2O5 (g) -> 2 N2O4 (g) + O2 (g).
Determine graphically the activation energy for the reaction. Attach graph to report.
T (K) | k (s^-1)
298 | 1.74 x 10^-5
308 | 6.61 x 10^-5
318 | 2.51 x 10^-4
328 | 7.59 x 10^-4
338 | 2.40 x 10^-3
Ea =
SUMMARY
Reaction Order | Differential Rate Law | Integrated Rate Law | Linear Plot | Slope of Linear Plot | Units of Rate Constant
0 | -d[A]/dt = k | [A] = [A]0 - kt | [A] versus t | - k | mol Lt^-1 sec^-1
1 | -d[A]/dt = k[A] | [A] = [A]0 e^-kt | ln [A] versus t | - k | s^-1
2 | -d[A]/dt = k[A]^2 | 1/[A] = 1/[A]0 + kt | 1 / [A] versus t | k | Lt mol^-1 sec^-1