Mechanisms and Molecularity < 7 of 18 > I Review | Constants | Periodic Table Part C Learning Goal: To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined. What is the rate law for step 1 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A]C type k* [A] + [C]^3. > View Available Hint(s) Very often, a reaction does not tell us the whole story. For instance, the reaction Rate = NO2(9) + CO(g)→NO(g) + CO2(g) does not involve a collision between an NO, molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: Submit 1. NO2(9) + NO2(9)→NO3(9) + NO(g) 2. NO3(g) + CO(g)→CO2(9) + NO2(9) Part D Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism. What is the rate law for step 2 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is kA||C type k* [A] * [C]^3. Overall, the resulting reaction is > View Available Hint(s) NO2(9) + CO(9)-→NO(g) + CO2(g) Rate

Mechanisms and Molecularity < 7 of 18 > I Review | Constants | Periodic Table Part C Learning Goal: To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined. What is the rate law for step 1 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A]C type k* [A] + [C]^3. > View Available Hint(s) Very often, a reaction does not tell us the whole story. For instance, the reaction Rate = NO2(9) + CO(g)→NO(g) + CO2(g) does not involve a collision between an NO, molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: Submit 1. NO2(9) + NO2(9)→NO3(9) + NO(g) 2. NO3(g) + CO(g)→CO2(9) + NO2(9) Part D Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism. What is the rate law for step 2 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is kA||C type k* [A] * [C]^3. Overall, the resulting reaction is > View Available Hint(s) NO2(9) + CO(9)-→NO(g) + CO2(g) Rate

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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1C. Effect of Catalyst Catalytic material to be tested Catalyst present (Yes or NO) Test Observation tube # Reference Clear solution, No fizzing (plain H2O2) NO 2 KI fast evolution Vigorous fizzing, gas/bubbles of yes yes NO Vigorous fizzing, Very fast evolution of gas/bubbles 3 PbO2 Copper wire No Change, No fizzing, No bubbles 5 Fresh potato Moderate fizzing, slow bubbles evolution yes yes Boiled potato Very slow fizzing, Few bubbles Which substance is the most catalytically active for H2O2 decomposition? Question 5. Arrange the five tested materials in order of increasing catalytic activity. Question 6. Explain for the difference in your observations between test tubes 5 and 6.
Chem 113-MC02 Spring 2021 View Available Hint(s) Cl(g) + CC (g) k. → CCL(g) (fast) ΑΣφ OA chemical reaction does not occur for this Submit Part B Complete previous partís) Part C Complete previous part(s) Copyright 2021 Person EducanAgns ved Provide Feedback ProblemiD=16204755480ffeet-prev
ST6D.1 (pre-exponential factor) - Determine the pre-exponential factor [in 1/(M s)] for a reaction with an activation energy of 3.9 kJ/mol if its rate constant equals 6.75/(M s) at 300 K. Hint = Draw a qualitative graph to see how to get b from the In(k) value you already have. Type your answer..
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+ Experimental Determination of a Rate Law 14 of 18 I Review | Constants | Periodic Tab Consider the reaction Part A A + 2B O What is the rate law for this reaction? whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Express the rate law symbolically in terms of k, [A], and [B]. • View Available Hint(s) [A] [B] Rate Trial (M) (M) (M/s) 0.40 0.050 9.6x10 3 ΑΣφ 1 0.40 0.100 1.9x10-2 rate = 3 0.80 0.050 3.8x10 2 Submit
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Question 30 of 39 Submit The zero order reaction A → Products takes 63.5 minutes for the concentration of A to decrease from 0.970 M to 0.205 M. What is the value of k for this reaction? M/min 1 3 4 C 7 8 9 +/- х 100 Tap here or pull up for additional resources
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