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

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter30: Kinetic Methods Of Analysis

Section: Chapter Questions

Problem 30.16QAP

See similar textbooks

Similar questions

The following results were found after completion of Part C in the Experimental procedure: 0.056 M I- and 0.048 M H2O2 were used Run Catalyst Calculated Rate of Reaction (M/s) 1 none 0.031 2 10.00mL of 0.35 M FeCl2 0.52 Assuming the Rate Law = k[I-][H2O2] 2 Calculate the value of k for run 2. Give your answer to the nearest whole number.
Table 2: Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20 Please help me with this part, and please show me all steps Order with respect to H2O2: Order with respect to KI:
If a mixture was prepared by diluting 7.0 mL of the Blue#1 solution with water to a final volume of 10.0 mL and mixing this with 2.0 mL of diluted bleach how many seconds would it require for the mixture to have an absorbance of 0.120? Use your measured values of b and of the average rate constant, k’ to answer this question. Show all work. Pls help me out asap!!
Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [?] (?) [?] (?)[) Rate (M/s) 1 0.370 0.390 0.0234 2 0.370 0.936 0.135 3 0.592 0.390 0.0374 ?= ? units= ?
Table 2: Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20 help me with this part please, and show me all steps Order with respect to H2O2: Order with respect to KI:
At 45 degrees Celsius, the N2O5 is monitored. Answer the data and determine the line's equation and R² and make the tables 3 and 4 are plotted in one graph. What is the slope of the line that is rate constant? Which model is the best?
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.360 0.290 0.0144 2 0.360 0.580 0.0144 3 0.720 0.290 0.0576 k=
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.360 0.330 0.0164 2 0.360 0.660 0.0164 3 0.720 0.330 0.0656 ?=? Units =?
Table 2: Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate(Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20 Order with respect to H2O2: -0.138 Order with respect to KI: -0.828 Rate constant value Trial 1: 5.84 Trial 2: 5.55 Trial 3: 5.56 Average: 5.6 -Please help me with this part, please 1. Should the rate constant (k) be the same for all three trials in this experiment? Explain your answer. 2.Write the complete rate law for this reaction.
Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.400 0.370 0.0216 2 0.400 0.962 0.146 3 0.600 0.370 0.0324 ?=
Describe type I mechanism in PDT? please asap within 15 min
Given the following data, determine the rate law and calculate K Experiment [NO] (M) [Cl2] (M) Rate (M/s) 1 0.0300 0.0100 3.4 x 10-4 2 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 10-4 the units on K are M-2s-1. You should enter the answer without units to 2 sig figs.