MISSED THIS? Watch KCV 14.5; Read Section 14.5. You canclick on the Review link to access the section in your e Text.The data below show the concentration of NaOs versus time forthe following reaction:Part ADetermine the order of the reaction,N,Os(g) - NO(g) + NO:(g)Time (s) N,Os (M)VOAE1.000250.822500.677750.5571000.458SubmitReauest Answer1250.3771500.310Part B Complete previous part(s)1750.2552000.210Part C Complete previous part(s)Provide Foodback

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The data below show the concentration of NaOs versus time for the following reaction: Part A N,Os(g) NO,(s) + NO,(g) Time (s) N,Os] (M) Determine the order of the reaction, 1.000 25 0.822 50 0.677 75 0.557 100 0.458 Submit Beauest Answer 125 0.377 150 0.310 Part B Complete previous part(a) (175 0.255 200 0.210 Part C Complete previous part(s) Provide Feedback

The data below show the concentration of NaOs versus time for the following reaction: Part A N,Os(g) NO,(s) + NO,(g) Time (s) N,Os] (M) Determine the order of the reaction, 1.000 25 0.822 50 0.677 75 0.557 100 0.458 Submit Beauest Answer 125 0.377 150 0.310 Part B Complete previous part(a) (175 0.255 200 0.210 Part C Complete previous part(s) Provide Feedback

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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See attached image for question A.) What is the order of the reaction in A? B.) What is the rate of reaction when the initial concentrations are [A]= 0 M and [B]= 4.4x 10-2M?
The following data were collected for the reaction: 2A > 4B + C Time Concentration of A Concentration of B (minutes) (moles/L) (moles/L) 1.000 0.000 10 0.800 0.400 20 0.667 0.677 30 0.571 0.858 40 0.500 1.000 50 0.444 1.112 1. Make a graph of the concentrations of A and B versus time. Estimate the rate of disappearance of A and the rate of formation of B at t= 25 min and at t= 40 min. Compare the rates of disappearance of A and formation of B. What would you expect the rate of formation of C to be at t= 25 min and t=40 min? 2. Determine graphically whether the reaction in #1 above is a first order or a second order reaction. Calculate the rate constant for the reaction.
Please don't provide handwritten solution ...
please add three grapgs, one graph of the order and anotheer two graphs that prove the order
17. SHOW ALL YOUR WORK OGiven the following data, determine the order of the reaction with respect to NO(g). 2 NO(g) + Cl2(g)→ 2 NOCI(g) Experiment 1 [C2] (M) 0.0100 [NO] (M) Rate (M/s) 3.4 x 104 1.36 x 103 3.4 x 104 0.0300 0.0150 0.0150 0.0100 3 0.0400
The reaction 2 NO (g) + O2 (g) → 2 NO2 (g) occurs when automobile exhaust releases NO into the atmosphere. Use the following data to determine the order with respect to NO for this reaction. Trial [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.012 0.020 1.02 x 10-4 2 0.024 0.020 4.08 x 10-4 3 0.024 0.040 8.16 x 10-4 Enter the answer as a single digit, not the word.
Experimental data for the reaction A + 2B → C have been plotted in the following three different ways. 0.05 -3.0 0.04 0.03 0.02 0.01 0 IvI 0 2 Time (s) 1/[A] 100 80 40 20 0 In[A] -3.5 -4.0 -4.5 -5.0 0 2 Time (s) 2 Time (s) What is the order of the reaction, and what was the initial concentration of A? O first-order, initial concentration = 10 M second-order, initial concentration = 10 M zero-order, initial concentration = 10 M O second-order, initial concentration = 0.1 M O first-order, initial concentration = 0.1 M
6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179
Determine the (a) rate law (b) solve for the order, and (c) value of rate constant for the reaction. C + D + E ⟶⟶ Products Reaction # [C]0 [D]0 [E]0 Initial rate (mol/L s) 1 0.400 0.300 0.560 7.14 x 10 -4 2 0.100 0.500 0.200 4.55 x 10 -5 3 0.100 0.200 0.200 4.55 x 10 -5 4 0.400 0.300 0.750 1.28 x 10 -3 5 0.100 0.300 0.560 3.57 x 10 -4
23 II. An experiment followed the decomposition. of nitregen dioxide to nitregen monoxide & oxygen gas. Given the following data, what order is the reaction for nitrogen dioxide? Given an initial concentration of nitrogen dioxide of 0.0400 M, what's the concentration of this reactant after a half hour? show all grapers & calcs to determine answers. (sec) Time |[NO₂] (M) 0.0 50.0 100.0 200.0 300.0 0.01000 0.00787 0.00649 0.00481 0.00380 M G 2 XX 6.5 Hoa X019 201 2(x) = 2 (1.86) (3 (9)
The following initial reaction rates have been measured for the following reaction NO2(g) + O3(g) -> NO3(g) + O2(g) Experiment: Initial Concentration (M) initial rate of the reaction O3 NO2 1 0.7 0.21 6.3 2 1.39 0.21 12.5 3 0.7 0.38 11.4 4 0.18 0.66 X a) Determine the order of and write the rate law of the reaction b) determine the value of K for the reaction. c) Find X
The following kinetic data were obtained for the reaction A (g) + 2 B (g) → products Trial [A] (M) [B] (M) Initial Rate (M s-1) 1 0.60 0.30 0.0126 2 0.20 0.30 0.0014 3 0.60 0.10 0.0042 Determine the order with respect to A. Enter the answer as a single digit, not the word.