Consider the following initial rate data (at 279 K) for the decomposition of a substrate (substrate 1) which decomposes to product 1 and product 2: [Substrate 1] Initial Rate 0.1 0.2 (M) (M/s) 0.00901 0.03604 0.6 0.32436 Determine the half-life for the decomposition of substrate 1 when the initial concentration of the substrate is 2.74 M.

The following data are for the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C. N₂O5 →→→→→2 NO₂ + ½ 02 [N₂05 ], M 0.200 0.100 5.00×10-2 time, min 0 133 266 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is 133 (2) Based on these data, the rate constant for this reaction is min -1 min. order 2.50×10-2 399

The decomposition of N2O5 occurs according to this reaction: 2 N2O5 (g) → 4 NO2 (g) + O2 (g) The following data about this reaction is collected: Time (min) [N2O5], M 0.0 0.400 1.0 0.385 5.0 0.332 10.0 0.276 20.0 0.190 30.0 0.131 40.0 0.090 a. Using Excel (or a similar program), determine the overall order of this reaction graphically. [You will need to create three separate graphs to determine the order.] Create a summary data table that shows what data was plotted (x-axis and y-axis), the equation for the best fit line, and the R2 value for each graph. b. Using the correct graph, report the value of k for this reaction.

the data in the table below were obtained for the reaction (see image) what is the magnitude of the rate constant for the reaaction

Determine the rate law for the reaction, 2IC1 + H2 = I, + 2HCi, from the following initial rate data: Initial Rate(Ms') 2.04x102 4.08x102 2.55x103 5.09x103 [H,], [ICI], 0.250 0.500 0.500 0.500 0.125 0.125 0.125 0.250 A) R = k[IC1]? В) R = k[H2]? C) R = k[ICI][H_]? D) R = k[ICl][H,] E) R = k[ICI]°[H¿] 000

Ozone in the stratosphere can be depleted in catalyzed reactions. The overall reaction for this exothermic process is given by: O3 +O→2O2, via the mechanism: NO+O3 →NO2 +O2 NO2 +O→NO+O2 Is this mechanism a chain reaction? Why or why not? Identify both the catalyst and the reactive intermediate in this mechanism. Draw to a relative scale the potential energy vs. reaction coordinate diagram for both the uncatalyzed reaction and the catalyzed reaction. Label transition states, activation energy, and reactive intermediates where appropriate.

0.1 M of a material has a decomposition rate constant (k) of 2.46×105 M-1 s-1. What equation would you use to calculate the half-life of decomposition?

Calculate the activation energy for the reaction (in kj/mol) when at 795 K the rate constant for the reaction shown below is 0.0000650, and at 370 K the rate constant is 0.00000300. 2N2O5(g) to 4NO(g) + 3O2(g)

Calculate the activation energy for the reaction (in kJ/mol) when at 675 K the rate constant for the reaction shown below is 0.0000860, and at 424 K the rate constant is 0.00000200 . 2N2O5(g)→4NO(g)+3O2(g)

For the gas phase decomposition of dichloroethane, CH3CHCI₂CH₂=CHCI + HCI the rate constant at 715 K is 9.93×10-4 s¹ and the rate constant at 756 K is 6.56×10-³ s¹¹. What is the activation energy for this reaction? kJ/mol