10 of 11Part AA certain reaction has an activation energy of 64.0 kJ/mol and a frequency factor of Aj = 8.90x102 What is the rate constant, k, of this reactionat 24.0 °C ?Express your answer numerically.> View Available Hint(s)Templates Symbols undo regdo Teset keyboard shortcuts helpk =SubmitThe linear form of the Arrhenius equationThe Arrhenius equation can be rearranged to a form that resembles the equation for a straight line:(수) (수) +In kIn Ambwhere y is In k, m is the slope orzİs , and b is the y-intercept or In A. The linearity of this equation is illustrated graphically in the image.(Figure 1)Part BAn unknown reaction was observed, and the following data were collected:T.(K)(M s352109426185Determine the activation energy for this reaction.Express your answer in kilojoules per mole.> View Available Hint(s)Templates Symbols undo redo feser keyboard shortcuts HelpkJ/molSubmitNext >Provide Feedback

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- Part A A certain reaction has an activation energy of 64.0 kJ/mol and a frequency factor of A, = 8,90x10 What is the rate constant, k, of this reaction at 24.0 °C ? Express your answer numerically. > View Available Hint(s) Templates Symbols undo PesEr keyboard shortcuts help redo Submit

- Part A A certain reaction has an activation energy of 64.0 kJ/mol and a frequency factor of A, = 8,90x10 What is the rate constant, k, of this reaction at 24.0 °C ? Express your answer numerically. > View Available Hint(s) Templates Symbols undo PesEr keyboard shortcuts help redo Submit

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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ST6D.3 - Given one billion collisions, how many collisions have sufficient energy to cause a reaction at 145.25°C if the activation energy is 50.0 kJ/mol? Type your answer...
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Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate = (8.98 × 10-4 ')[c,os] -1 S Suppose a vessel contains Cl₂05 at a concentration of 1.40M. Calculate the concentration of Cl₂O5 in the vessel 690. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
ANSWER TWO PLS
*Determine the Activation Energy for the reaction in both Joules per mole and Kilojoules per mole*Determine the frequency factor (A) for the reaction *Determine the rate constant at 10.0ºC, *Determine the rate constant at 30.0ºC.*If you start the reaction with [C2H5Br] = 0.155M and [OH-] = 0.250M what is the initial rate of the reaction at 10.0ºC and at 30.0ºC.
The following initial rate data are for the reaction of ICI with hydrogen: 2IC1 + H₂ → I₂ + 2HCl Experiment [IC]o, M [H₂], M 0.198 0.141 0.396 0.141 0.198 0.281 0.396 0.281 1 2 3 4 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 = k = -2 M-². Initial Rate, M. s-¹ S 0.00657 0.0131 0.0261 0.0522 -1 S
The rate of a certain reaction is given by the following rate law: rate =k| N,| H2 -k[N;][H+]° Use this information to answer the questions below. What is the reaction order in N,? What is the reaction order in H2? What is overall reaction order? At a certain concentration of N, and H2, the initial rate of reaction is 0.620 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 24.0 M / s when [N2] = 1.5 M and [H2] = 0.16 M. Calculate the value of the k = |M -2 -1 •S rate constant. Round your answer to 2 significant digits.
A particular reactant decomposes with a half-life of 121 s when its initial concentration is 0.354 M. The same reactant decomposes with a half-life of 239 s when its initial concentration is 0.179 M. Determine the reaction order. 01 What is the value and units of the rate constant for this reaction? Units 0.17 Enter numeric value TOOLS x10