2. Consider the following reaction: Time b) What is the rate law? 0 1000 2000 3000 4000 5000 A B [A] (M) 0.475 0.350 0.277 0.230 0.196 0.171 a) Determine the order of the reaction by graphing the data appropriately. You may create graphs by hand using the graph paper provided or by using Excel or Google Sheets (be sure to include an image of your graph). Explain your answer. c) What is the rate constant? Provide appropriate units.

2. Consider the following reaction: Time b) What is the rate law? 0 1000 2000 3000 4000 5000 A B [A] (M) 0.475 0.350 0.277 0.230 0.196 0.171 a) Determine the order of the reaction by graphing the data appropriately. You may create graphs by hand using the graph paper provided or by using Excel or Google Sheets (be sure to include an image of your graph). Explain your answer. c) What is the rate constant? Provide appropriate units.

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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7. The rate of the reaction NO,(g) + CO(g) → NO(g) + CO,(g) depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected: Time (s) [NO,] (mol/L) 0.500 1.20 X 103 3.00 X 103 0.444 0.381 4.50 X 103 0.340 9.00 X 103 0.250 1.80 X 104 0.174 Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [NO2] at 2.70 × 10* s after the start of the reaction.
Given the following rate and concentration data, determine the rate law for the reaction A + B ---> products [A]0 (M) [B]0 (M) initial rate (M/s) 0.10 0.10 4.22 X 10^-6 0.20 0.10 8.44 X 10^-6 0.20 0.40 3.38 X 10^-6 the rate constant k= rate=
Consider the following reaction: Cl2O (g) + CO (g) → Cl2 (g) + CO2 (g) Initial rate of the reaction was measured at multiple different concentrations of CO, which created the following data: [CO] (M) Initial Rate (M/s) 0.10 0.0020 0.20 0.0040 0.40 0.0080 From this data, we can see that the reaction order with respect to CO is __________. Consider the following reaction: Cl2O (g) + CO (g) → Cl2 (g) + CO2 (g) Initial rate of the reaction was measured at multiple different concentrations of CO, which created the following data: From this data, we can see that the reaction order with respect to CO is __________. a. 1st Order b. 3rd Order c. 2nd Order d. 0th Order
Consider this reaction: A + B → C + D Expt. [A] (M) [B] (M) Initial Rate (M/s) 1 0.100 0.100 0.152 2 0.100 0.200 0.152 3 0.200 0.200 0.305 What is the overall reaction order for this reaction?
Consider this reaction: 2HI (g) → H₂ (g) + 1₂ (g) At a certain temperature it obeys this rate law. rate = (0.00315 M¹-s¯¹) [HI] ² S olo Suppose a vessel contains HI at a concentration of 1.16M. Calculate the concentration of HI in the vessel 970. seconds later. You may assume no other reaction is important. Ar Round your answer to 2 significant digits. M x10 X Ś ?
The following initial rate data was obtained for the reaction between oxygen and nitric oxide. 2 NO(g) + O₂(g) → 2 NO2(g) [0₂] (M) [NO] (M) Rate (M s-¹) 0.0100 0.0150 0.0150 0.0100 0.0100 0.0200 10.0 22.5 45.0 J What is the rate law for this reaction under these conditions? Rate = k [0₂]2 [NO]² Rate = k [0₂] [NO]² Rate = k [0₂]²2 [NO] Rate = k [0₂] [NO] G
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Very confused with this rate law
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