NO is an atmospheric pollutant that destroys ozone in the stratosphere. Here is the accepted mechanism:Оз+ NO+ NO2 + O2 (slow)NO2 + O + NO + O2 (fast)Оз+0 —- 202X Incorrect.Identify any catalyst in the mechanism. If none, enter none.EditnoneeTextbook and MediaCorrect.Identify any intermediate in the mechanism. If none, enter none.NO,

Given reaction mechanism: We have to find the catalyst and the intermediate.

NO is an atmospheric pollutant that destroys ozone in the stratosphere. Here is the accepted mechanism: O3+ NO + NO2 + O2 (slow) NO2 +O + NO + O2 (fast) O3 +0 → 202 X Incorrect. Identify any catalyst in the mechanism. If none, enter none. Edit none eTextbook and Media Correct. Identify any intermediate in the mechanism. If none, enter none. NO,

NO is an atmospheric pollutant that destroys ozone in the stratosphere. Here is the accepted mechanism: O3+ NO + NO2 + O2 (slow) NO2 +O + NO + O2 (fast) O3 +0 → 202 X Incorrect. Identify any catalyst in the mechanism. If none, enter none. Edit none eTextbook and Media Correct. Identify any intermediate in the mechanism. If none, enter none. NO,

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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Calculate the rate constant considering the following rate data obtained at 25oC for the following reaction.
5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.
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
Consider the following reaction mechanism. Step 1 : W2 ⇌ 2W (fast) Step 2 : W + Z ⇌ D + F (fast) Step 3 : W + F → M (slow)Write the predicted rate law
X Cut AaBbCcl AaBbCcDc AaBbCcD AaBbCcE AaB AaBb CcC Aa8be T No Spac. Heading 2 Calibri (Body) | AA Aa. E , 刻T Copy Paste Subtle Title Subtitle BIU abc x, x A - y- A- Heading 1 T Normal Format Painter Paragraph Styles Font Clipboard I 10 11 6. From the data variation of the reaction rate of the following temperatures: 1500 T (K) k (M1 second ) 500 1000 5,49 x 106 9,86 x 108 5,09 x 10° Specify: a. Amount of Activation Energy (Ea) b. Magnitude of the pre-exponential factor (A)
A certain reaction is second order in N, and first order in H₂. Use this information to complete the table below. Round each of your answers to 3 significant digits. [₂] 1.94 M 1.94 M 3.73 M 1.34 M 6.33 M 0.697 M initial rate of reaction 0.349 M/s M/S M/S X
Analyze the following reaction mechanism: 1. H2O2 → H20 + O H2O + O 2. O + CF2CI2 → CIO + CF2CI 3. CIO + Oз — CI + 202 4. CI + CF2CI → CF2CI2 Identify the catalyst in this reaction. A) O3 B) O2 C) H2O2 D) CF2CI E) CF2CI2
For the following chemical Konction there are possible Reaction mechanisms as Shown STEP I Step 2 NET 2 co + Cl₂ → 2 Coll STEP 1 Step 2 REACTION MECHANISM I со - CO + Cl₂ ⇒ Coll + el C(Slow) (Fast) со coel اح tee Three MECHANISM I Cl₂ → 2 l (Slow) llz 2 ll + 10 + 2 coll (Fast)
5.
The following mechanism has been proposed for the reaction of H2 (g) and NO (g): H2 (g) + NO (g) → H2O (g) + N (g) (Slow)N (g) + NO (g) → N2 (g) + O (g) (Fast)H2 (g) + O (g) → H2O (g) (Fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.
10. The data below are for the reaction: 2 NO₂ (g) + F₂ (g) → 2 NO₂F (g) [NO₂] (M) 0.100 0.200 0.200 0.400 0.200 [F₂] (M) 0.100 0.100 0.200 0.400 0.400 Initial rate (M/s) 0.026 0.051 0.103 0.411 see part c a. Write the rate law for this reaction. b. Determine the rate constant for this reaction. Pay attention to units. c. Predict the initial rate of the reaction when [NO₂] = 0.200 M and [F₂] = 0.400 M. d. The mechanism of the reaction is suggested as two steps: NO₂+ F2 → NO₂F + F (fast) NO₂+ F→→ NO₂F (slow) Is your rate law consistent with this mechanism? Explain your answer, making any changes necessary to create consistency.
The rate of disappearance of HBr in the gas phase reaction 2HBr (g) is 0.301 M s-¹ at 150°C. The rate of appearance of Br₂ is 1.66 0.151 H2(g) + Br2 (g) 0.0906 0.602 0.549 M s-¹.