For your temperature studies in Part Ba student obtain the results below for the temperatures and rate constants. Calculate the activation energy in units of kJ/mol. Data Table Temperature (°C) Rate constant (k, appropriate units based on reaction order) 17 6,689,537,124 41.8 18,563,418,549 2.1 1,247,348,345 Note: The easiest way to do this is by creating a plot in Excel, as you will do in lab. These numbers are made up, and will be different from those you determine in lab. Report your answer with one place after the decimal.

A particular 1st-order reaction with a single reactant, whose initial concentration is 0.87 M, has a rate constant of 8.54 s–1. Determine t½ for this reaction. Group of answer choices 0.31 0.089 1.8 1.3 0.081

6. The rate constants for the decomposition of a compound are 6.2 x 10* s' at 45°C and 2.1 x 103 s1 at 55°C. What is the value of the activation energy for this reaction in kJ/mol? А. 1.7 х 10% В. 1.1 x 105 C. 2.5 x 103 D. 2.5 x 104 E. 1.1x 106

Which statement best describes the image?  This image illustrates the calculation of an instantaneous rate for the product. This image illustrates the calculation of an average rate for the product. This image illustrates the calculation of an average rate for the product. This image illustrates the calculation of an instantaneous rate for the reactant.

Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A] (M) 0.00 0.450 0.50 0.300 1.00 0.225 1.50 0.180 2.00 0.150 2.50 0.130 3.00 0.115 3.50 0.100 4.00 0.090

Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A](M) 0 0.5 1.5 0.42 3 0.335 4.5 0.25 6 0.17 7.5 0.085 9 0.003

1. indicate the activation energy for the overall reaction on the graph. (You may want to use a line for the sake of clarity.)2. Write the elementary reactions that make up the reaction mechanism. 3. What would you propose as the rate law for this reaction? 4. Of course, this proposed law is hypothetical. Using the following data collected experimentally (probably using a UV/vis spectrometer J), determine the rate law for this reaction. Include reaction order and the value and units for k. Please show your work, including any graphs you make. (Note: no credit will be given to correct final answers without supporting work.) Does your experimental rate law match the one you proposed above?

General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Initial-rate data at a certain temperature is given in the table for the reaction N,0,(g) NO(g) + NO,(g) [N,O,], (M) Initial rate (M/s) 0.100 0.480 0.200 0.9600 0.300 1.440 Determine the value and units of the rate constant. units: k =