5. Which of the following statements best describe the overall order of the reaction? 0.015 0 30 60 90 120 150 0 30 60 90 120 150 Time (s) Tlmelgl ཡང་། ང་ 0.035 120 150 Time (s) zeroth order due to the [C5H6] decreasing over time which indicates reactants being consumed first order due to the plot of In[C5H6] over time and slow decrease over time second order due to the linear plot of the inverse [C5H6] over time

Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+ 2B C+D k = Trial [A] (M) [B] (M) Rate (M/s) 1 0.320 0.360 0.0123 2 0.320 0.720 0.0123 3 0.640 0.360 0.0492 Units

Initial‑rate data at a certain temperature is given in the table for the reaction SO2Cl2(g)⟶SO2(g)+Cl2(g)   [??2??2]0(?)[SO2Cl2]0(M) Initial rate (M/s) 0.100 2.30×10−62.30×10−6 0.200 4.60×10−64.60×10−6 0.300 6.90×10−6   Determine the value and units of the rate constant.     ?=     units:

The following initial rate data are for the gas phase reaction of hydrogen with iodine: H₂+I2 → 2 HI Experiment [H₂]o, M 0.0464 0.0464 1 2 3 4 k 0.0928 0.0928 = -1 Initial Rate, M-s-¹ [2]o, M 0.00461 0.00923 0.00461 8.17 x 10-22 0.00923 1.64 x 10-21 M-¹.8-¹ Complete the rate law for this reaction in the box below. Use the form k[A]™ [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = -22 4.09 x 10 8.18 × 10-22

Using the data in the table, determine the rate constant of the Trial [A] (M) | [B] (M) | Rate (M/s) reaction and select the appropriate units. 1 0.330 0.330 0.0123 2 0.330 0.660 0.0123 A + 2B C + D > 3 0.660 0.330 0.0492 Units k = SТOOLS x10

The table gives the concentrations of NO, (g) as a function of time at a certain [NO2] (M) time (s) temperature for the reaction 0.0831 0.0 0.0666 4.2 NO, (g) → NO(g) + 0,(g) 2 0.0567 7.9 1 Verify that this is a second-order reaction by plotting NO versus time and [NO,] 0.0497 11.4 determining the value of the rate constant. 0.0441 15.0 k = M-1 . s-1

Data is collected for the gas phase reaction 2 A + B + 3 C → Products at 470 K. What is the order of the reaction with respect to A?

Order and rate law of a reaction The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is rate = k[NO₂)² The exponent "2" is used because the reaction involves two NO₂ molecules. The rate law for step 2 is because the reaction involves only one molecule of each reactant the exponents are omitted. Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1.2A B+C 2. B+D+E+C Part A What is the overall reaction? Express your answer as a chemical equation. ► View Available Hint(s) for Part A for Pardo for Part redo foPart A refor Part A keyboard shortcuts for Part A help for Part A A chemical reaction does not occur for this question. Submit Part B Which species is a reaction…

Analyze the following mechanism: What are the intermediates and catalysts if there are any? What is the overall reaction?

Using the kinetics data below, determine the orders for A,B, and C. Write the rate law. Then determine the value and units of the rate constant. Trials Initial [A] (M) Initial [B] (M) Initial [C] (M) Initial Rate (M/s) 1 0.30 0.50 0.050 1.6 x 10-6 2 0.10 0.25 0.050 3.9 x 10-7 3 0.30 0.25 0.050 3.9 x 10-7 4 0.30 0.50 0.10 6.3 x 10-6 Orders [A] ________, [B] _________, [C] _________ Rate Law: ____________________________________________________ Rate Law constant with units : ______________________________