5) NO2(g), (a.k.a. smog! And I don't mean the dragon), reacts with and causes the decayof ozone.Determine the rate law and the value of k for the following reaction using the dataprovided.NO2(g) +03(g) → NO3(g) + O2(g)[NO2]i (M)[03]i (M)Initial Rate0.100.331.420.100.660.250.662.847.10FULL ANSWER:6) A data for the reaction in #5 was from experiments performed at room temperature(assume 25 °C). The energy of activation of the reaction is 63 kJ/mole.Use the rate constant you determined above to discover rate constant at -3 °C, which isthe temperature of the stratosphere.ANSWER:

5)Rate law:rate = k[NO2][O3]rate constant:43.0 M−1⋅s−16) rate constant at −3∘C=3.08…

Answered: 5) NO2(g), (a.k.a. smog! And I don't…

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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Consider this reaction: H,CO, (ag) → H,0 (aq)+CO, (aq) At a certain temperature it obeys this rate law. rate = (0.0261 s')[H,Co,] [H,Co.] Suppose a vessel contains H,CO, at a concentration of 0.390M. Calculate the concentration of H,CO, in the vessel 40.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 Continue Submit Assign 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Acces MacBook Air 80 DII DD F1 F3 F4 F5 F6 F7 F8 F9 F10
rate?
A particular reactant decomposes with a half-life of 173 s when its initial concentration is 0.301 M. The same reactant decomposes with a half-life of 231 s when its initial concentration is 0.225 M. Determine the reaction order. 01 0 2 What is the value and units of the rate constant for this reaction? k = Units
3. An experiment was carried out to determine the rate law for the following reaction: 19152 2NO( )+0( ) → 2NO( ) Where the rate law is: par Rate = k[NO] [0] The experiment was repeated three times and the following data recorded: Experiment # Initial [NO] (M) Initial [0] (M) Rate (M/s) 1 ullo2 M0.015 0.015 2 0.030 0.015 3 0.015 0.030 of in Determine the value of x in the rate law (order of reaction with respect to NO) by comparing experiments 1 and 2 in Equation 13 reaction with respect to O₂) by comparing experiments 1 and 3 in equation 13. 0.048 0.192 0.096
Can you explain the concept? How to apply the concept to this problem and other problems?
The decomposition of nitrosyl bromide is followed 2 NOBr → 2 NO + Br2 Time (s) [NOBr] (M) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033 Determine the average rate over the entire experiment.
Given- H2S (g) + O2 (g) → H2O (g) + S8 (g)-Write the expression of the rate in terms of the concentration of eachreactant and product over time.-If the rate of formation of S8 is 0.078 M/s, what is the rate ofdisappearance of H2S?
consider the reaction 2 H2 (g) + O2 (g) = 2H2O (g). Determine the rate in which H2O is formed
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. 1 rate = (0.471 M¹S -¹) [N₂05]² Suppose a vessel contains N₂O5 at a concentration of 0.800M. Calculate the concentration of N₂O5 in the vessel 8.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10
for the reaction between nitrogen monoxide and chlorine to produce nitrosyl chloride 2NO + Cl2 --> 2NOCl it is found that tripling the concentration of both reactants increases the rate by a factor of 27. if only the concentration of chlorine is tripled the rate increases by a factor of 3. give order of this reaction with respect to NO and determine the rate law for the reaction
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A particular reactant decomposes with a half‑life of 117 s117 s when its initial concentration is 0.376 M.0.376 M. The same reactant decomposes with a half‑life of 221 s221 s when its initial concentration is 0.199 M.0.199 M. Determine the reaction order. 2 1 0 What is the value and units of the rate constant for this reaction? ?=k= Units

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