Reaction rates and rate laws for the following gas phase reaction are given. [03] = 1.0 × 10¹4 molecules/cm³ Time (ms) [NO] 0 6.0 x 108 100 5.0 x 108 500 2.4 × 108 700 1.7 x 108 1000 9.9 × 107 Using the data above: a. Graph concentration vs. time for each data set. b. Graph In[] vs. time. c. Determine the average rate for the reaction between each data point. NO(g) +O3(g) → NO₂(g) + O2(g) [NO]=2.0 x 10¹4 molecules/cm Time [03] 0 1.0 × 10¹⁰ 50 8.4 x 10⁹ 100 7.0 x 10⁹ 200 4.9 x 10⁹ 300 3.4 x 10⁹

Reaction rates and rate laws for the following gas phase reaction are given. [03] = 1.0 × 10¹4 molecules/cm³ Time (ms) [NO] 0 6.0 x 108 100 5.0 x 108 500 2.4 × 108 700 1.7 x 108 1000 9.9 × 107 Using the data above: a. Graph concentration vs. time for each data set. b. Graph In[] vs. time. c. Determine the average rate for the reaction between each data point. NO(g) +O3(g) → NO₂(g) + O2(g) [NO]=2.0 x 10¹4 molecules/cm Time [03] 0 1.0 × 10¹⁰ 50 8.4 x 10⁹ 100 7.0 x 10⁹ 200 4.9 x 10⁹ 300 3.4 x 10⁹

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...

See similar textbooks

Similar questions

A particular reaction is proposed to be first order. What plot would support this conclusion? a. a linear plot of [reactant] versus time b. an exponential decay of [reactant] versus time c. a linear plot of ln [reactant] versus time d. an exponential decay of ln [reactant] versus time
grade 12 chem: textbook question please show all work and answers must have correct units and significant figures.
5. A laboratory experiment was done for the reaction below and the following data was obtained: A→ Products a. Reaction order. Time (hours) Concentration of A, mg/L 0 1 Plot the data in Excel and determine the following: b. Reaction rate, k. 23468 135 119 104 88 73 41 10
Consider the following reaction: C6H11F + KBr → C6H11B1 + KF The following concentration vs. time data were collected. [CH11E]. time. min 0.400 M 0.380 M 3.00 0.350 M 7.70 0.320 M 12.87 0.300 M 16.32 0.270 M 22.64 0.250 M 27.24 A. Graph the data to determine the order. B. What is the order with respect to [C6H11F]? C. Calculate the rate constant, k. D. Write the rate law (equation). E. Calculate the half-life. F. How many minutes will it take to reach a concentration of 0.280 M? Upload the graphs with correlation coefficients and trendline equations and calculations.
Car note CAU EMAIL CANVAS Pirate Ship MYJSCC BLACKBOARD Vacancies | A...| Birmingham Paraphrasing ...ewriting Tool Bb Content C OWLV2 | Online teaching and learning resour Students Home [References] Use the References to access important values if needed for this question. The following initial rate data are for the reaction of nitrogen dioxide with fluorine: 2 NO2 + F2 → 2 NO,F Experiment [NO2]0, M [F2]o, M Initial Rate, Ms 1 2.96 0.762 2.53x10-4 2.96 1.52 5.04x10-4 3 5.92 0.762 5.05x10-4 4 5.92 1.52 1.01x103 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = %3D From these data, the rate constant is Mls1. Submit Answer Try Another Version 1 item attempt remaining
8) A first order reaction starts with a concentration of reactant equal to 0.040 M. After two hours, the molarity is 0.020M. What is the molarity after four hours? a. 0.015M c. 0.005M e.0.03 М b. 0.010 M d.0.0025 M
17. A first order decomposition reaction was found to have an initial rate of 0.19 M-min- when the initial reactant concentration was 0.33 M. What is the initial rate of reaction if the initial concentration is increased to 0.45 M? D. 0.19 M·min E. 0.58 M·min- A. 0.26 M·min- B. 1.3 M-min¬1 C. 0.78 M·min-
. For the following generic reaction: a A + b B -- > c C + d DWhat is the rate of reaction (rate expression) as a function of change in concentration (e.g. Δ[A]) andchange in time (Δt)?Describing Chemical Kinetics:1. Measuring RateThe rate of a chemical reaction is determined by:A. Change of moles of reactants/products over change in timeB. Change of grams of reactants/products over change in timeC. Change in concentration over change in timeD. change in volume over change in timeWrite the rate expressions based on the definition above for:a A + b B -- > c C + d Da A -- > productsDoes the order in reactant (m, n) in the rate law have anything to do with the coefficients of the reactants?