Consider the reaction: NO2 + O3 -> NO3 + O2 Experiment [NO2], M [O3], M Rate, M/s Trial 1 0.21 0.70 6.30x10-3 Trial 2 0.63 0.65 1.89x10-2 Trial 3 0.21 0.35 3.15x10-3 Trial 4 0.42 0.35 6.30x10-3 A) Which experimental trial expressed the rate order of NO2? B) Which experimental trial expressed the rate order of O3? C) What is the rate order of O3? D) What is the rate order of NO2? E) What is the overall rate reaction?

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= For a different reaction X2Y, the initial [X] 1.0 M, and [Y] = 0 M. After 5 minutes the [X] has fallen to 0.8 M and then does not change any further. Draw a graph of [X] v time for the first 10 minutes. Use the blank template graph from Q1. Use the editor to format your answer

Use this data for the following four (4) questions: The relative initial rates of the reaction A2 + B2-products in vessels (a)-(d) are 1:1:4:4. The spheres represent the number of molecules of present at the beginning of the reaction. [Unshaded spheres = A2 molecules; shaded spheres = B2 molecules] %3D For example, vessel (a) contains 2 A2 molecules and 2 B2 at the beginning of the reaction. Rate = 1 Rate 1 Rate = 4 Rate = 4 %3D 2. 8. 80 (c) (a) 11) What is the order of reaction with respect to A2? (b) (d) BA 11) A))0 B) 1 C) 2 D) 3 12) What is the order of reaction with respect to B2? 12) C A) 0 B) 1 D) 3 13) o c 13) What is the overall order of reaction? A) 0 B) 1 D) B 14) 14) What is the rate law for this reaction? B) Rate k[B2]2 D) Rate = k[A2]2[B2]² A) Rate = k[A2]² %3D C) Rate = k[A2][B2] %3D %3D nation below: 15) 8. 8.

The following is the concentrations of the reactants and products as function of time for the reaction below: 2 NO2(g) Molar concentration 0.012 0.01 0.008 0.006 0.004 0.002 700 690 680 670 660 650 640 630 620 610 600 590 580 570 560 550 540 530 520 510 500 Time (sec) [NO₂] [NO] [0₂] 0.0100 0.0000 0.0000 490 480 470 (a) Plot the [NO₂], [NO], [O₂] vs. time all on same chart. (b) Label the appropriate chart title, x-axis, y-axis, (review charting guidelines) (c) Distinguish the three curves by making the [NO₂] curve as solid line, the [NO] curve as broken line and the [O₂] curve as dotted line. See the following graph for demonstration. 460 450 0 50 100 150 200 250 300 350 400 0 0.0079 0.0021 0.0011 0.0065 0.0035 0.0018 100 0.0055 0.0045 0.0023 0.0048 0.0052 0.0026 0.0043 0.0057 0.0038 0.0062 A Plot of Reactant and product concentrations vs. Time The absorbance spectrum of the [Co(NH3),CO3] complex is given below Wavelength (2, nm) Absorbance A Aabs. 2 NO(g) + O2(g) at 573 K 0.0034…

2. For the following reaction at 500 °C Cl2 (g) + H2 (g) 2 HCI (g) + the following data were collected: Experiment [H2 ] [ Cl2 ] Initial Reaction Rate 1 0.025 M 0.012 M 1.60 x 10 4 2 0.050 M 0.012 M 6.40 x 10 -4 3 0.050 M 0.048 M 6.40 x 10 -4 Give a rate law expression for this reaction and also calculate the value of the rate constant (k) for this reaction. What is the overall order of this reaction?

23. The following data were measured for the reaction BF3(g) + NH3(g) ---> F3BNH3(g) Experiment [BF3] (M) [NH3] (M)  initial rate (M/s) 1 0.250 0.250 0.2130 2 0.250 0.125 0.1065 3 0.200 0.100 0.0682 4 0.350 0.100 0.1193 5 0.175 0.100 0.0596 What is the overall order of the reaction? Group of answer choices A. 3 B. 2 C. 1 D. 0

Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [02], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 × 10-2 3.15 x 10-3 2 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2land 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.

The data below show the concentration of cyclobutane (C4H8) versus time for the following reaction: C4H8→2C2H4 Time (s) [C4H8] (M) 0 1.000 10 0.894 20 0.799 30 0.714 40 0.638 50 0.571 60 0.510 70 0.456 80 0.408 90 0.364 100 0.326 What is the rate of reaction when [C4H8]= 0.26 M ? Express your answer using two significant figures. Please show how to do this question and find the rate law without graphing it. Thank you.

Consider the following reaction: CaO(s) + CO₂(g) → CaCO3(s) The data found below are the results obtained from using different concentrations of each reactant to measure the initial rate of the reaction: Trial 1 2 3 4 [CaO] (mol L-¹) [CO₂] (mol L-¹) 0.0050 0.0150 0.0200 0.0150 0.0020 O 0.0021 mol L-1 O 0.0042 x 10-² mol L-¹ O 0.4167 mol L-1 O 0.0083 mol L-1 O 0.004 mol L-1 0.0020 0.0040 Determine the concentration of CO₂ during trial 3. Initial Rate (mol L-¹ s-¹) 1.50 × 10-3 0.0135 0.025 0.027