The tabulated data were collected for this reaction at 322 K:A(9) → B(9)Тime(min.)[A] (M)5.251.51166.301.25967.871.00779.260.856610.500.755815.750.503921.000.377926.250.302331.500.251936.750.215942.000.1889Determine the average rate of this reaction between 5.25 min. and 7.87 min.:average rate(M/min)humber (rtol=0.03, atol=1e-08)e x 0%

Rate of reaction is change in concentration of products or reactant in given time interval Average…

:5 1.5116 1.2596 =7 1.0077 0.8566 50 0.7558 75 0.5039 0.3779 25 0.3023 50 0.2519 75 0.2159 D0 0.1889 erage rate of this reaction between 5.25 min. and 7.87 min.: (M/min) = humber (rtol=D0.03, atol=1e-08) e x0%

:5 1.5116 1.2596 =7 1.0077 0.8566 50 0.7558 75 0.5039 0.3779 25 0.3023 50 0.2519 75 0.2159 D0 0.1889 erage rate of this reaction between 5.25 min. and 7.87 min.: (M/min) = humber (rtol=D0.03, atol=1e-08) e x0%

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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B IU Av A 1. Using the Ideal Gas Law (PV = nRT), calculate the grams of O2 produced in the reaction. Show %3D your work and follow the steps below. If you pressure is not yet in atm, convert it to atm using the appropriate conversion factor. b. Convert the volume of oxygen collected from mL to L. C. Convert the temperature of the water from °C to K. d. Plug in P, V, R (gas constant), and T to the ideal gas law and solve for n, which is moles of oxygen gas. e. Use the moles of oxygen gas found and the molar mass of O2 to calculate the grams of oxygen produced using dimensional analysis.
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3. Using the following data below for the reaction of AB A+ B Time (sec) [AB] (M) 0.0 4.77 x 104 1.00 2.00 3.00 5.00 10.00 30.00 -50.00 4.31 x 104 3.91 x 104 3.53 x 104 2.89 x 104 1.76 x 10-4 2.4 x 10-5 3.2 x 10-6 a. Plot the data shown and determine what order the reaction b. Calculate the k value for this reaction. C. What is the half-life for this reaction? d. What is the concentration of AB after 40 seconds?
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For the reaction 2 NO(g) + O 2 (g) → 2 NO2 (g) have the following data. Experiment 1 2 3: [NO], M 0.010: 0.020: 0.010 [O 2 ], M 0.010 :0.010: 0.020 The speed of consumption of 2.5 x 10-5 1.0 x 10-4 5.0 x 10-5 NO, Ms -1 a) write the rate equation for the reaction b) calculate the rate constant
estion 3 of 3 Time and concentration data were collected for the reaction 0.52 A → products 0.48 0.44- t (s) [A] (M) 0. 0.52 0.40- 20 0.43 0.36- 40 0.35 0.32- 60 0.29 0.28 - 80 0.23 100 0.19 0.24 0.20. The blue curve is the plot of the data. The straight orange line is tangent to the blue curve at t = 40 s. 0.16. 0 10 20 30 40 50 60 70 80 90 t (s) Approximate the instantaneous rate of this reaction at time t = 40 s. instantaneous rate: M/s [A] (M)
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With complete rate law. Finish finding m to add to n for overall reaction then find complete rate law.
Expt. 1 2 3 NH; (aq) + NO; (aq) >Nz (aq) + 2 H2O (l) [NO₂] Rate (at 298 K) 0.020 M/s 0.020 M 0.020 M 0.030 M/s 0.010 M 0.0050 M/s [NH+] 0.010 M 0.015 M 0.010 M Determine the complete rate law (rate law and rate constant) for the reaction. Show all work. What is the initial rate of this reaction if the concentrations in Expt. 2 above are tripled. Show work. What is the rate of H₂O formation in Expt. 1? A 4th trial is conducted at 273 K, using the concentrations from Expt. 1. If the rate was found to be 0.016 M/s, calculate the activation energy of this reaction.
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