The activation energy for a certain first order reaction is 139 kJ/mol. If the rate constant is 0.282 sat 12.4°C, what will the rate constant for the reaction be if the temperature is doubled? (A) (B) (C) (D) (E) 0.564 s1 0.283 s1 0.361 s1 0.553 s1 3.22 s1

The activation energy for a certain first order reaction is 139 kJ/mol. If the rate constant is 0.282 sat 12.4°C, what will the rate constant for the reaction be if the temperature is doubled? (A) (B) (C) (D) (E) 0.564 s1 0.283 s1 0.361 s1 0.553 s1 3.22 s1

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

For the decomposition of gaseous dinitrogen pentaoxide,2N₂O₅(g) →4NO₂(g) +O₂(g), the rate constant is k=2.8X10⁻³ s⁻¹at 60°C. The initial concentration of N₂O₅ is1.58 mol/L. (a) What is [N₂O₅] after 5.00 min? (b) What frac-tion of the N₂O₅ has decomposed after 5.00 min?
The radioactive isotope 28Mg has a half-life of 20.9 hours. (a) What is the rate constant for this first-order reaction? (b) What fraction of the isotope remains after 24 hours? Assume 3 significant figures in your calculations.
1a) Calculate the rate constant (with appropriate units) for a first order reaction which is 32.0% complete in 380 s. 1b) What is the value of the half-life of the reaction? 1c) How long will it take for the reaction to go to 76.0% completion?
Iodine atoms combine to form molecular iodine in the gas phase This reaction follows second-order kinetics and has the high rate constant 7.0 x 10°/M s at 23°C. If the initial concentration of I is 0.086 M, calculate the concentration after 2.0 min. (a) (b) Calculate the half-life of the reaction if the initial concentration of I is 0.60 M and if it is 0.42 M. B Strategy (a) I(g) + I(g) → 12 (8) (b) 1 1+1—h Page 589 The relationship between the concentrations of a reactant at different times is given by the integrated rate law. Because this is a second-order reaction, we use Equation (13.7). We are asked to calculate the half-life. The half-life for a second-order reaction is given by Equation (13.8).
Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s-1. (a) What is the half-life for this reaction? _______ s(b) If you start with 0.047 M I2 at this temperature, how much will remain after 5.18 s assuming that the iodine atoms do not recombine to form I2? _______ M
1) The half-life for a first-order reaction, A→B is 7.75 s. If the initial [A] is 0.75 M, how long will it take for [A] to reach 0.60 M. 2) The decomposition of O3 is a second order reaction with a rate constant of 50.5 M hr-1. 2O3(g)→3O2(g) What is the half-life for the decomposition of O3 when the concentration of O3 is 5.609 x 10-6 M?
The initial rate of the reaction is determined for different initial conditions, with the results listed in the table. (a) What is the overall reaction order? (b) What is the value of the rate constant, k
As described in Exercise 14.41, the decomposition of sulfuryl chloride 1SO2Cl22 is a first-order process. The rate constant for the decomposition at 660 K is 4.5 * 10-2 s-1. (a) If we begin with an initial SO2Cl2 pressure of 450 torr, what is the partial pressure of this substance after 60 s?
Consider the following reaction: 1. 2 N,O5 (g) → 4 NO, (g) + O, (g) The initial concentration of N2O5 was 0.48 mol/L, and 25 minutes after initiating the reaction, all of the N,Os has been consumed. (a) Calculate the average rate of the reaction over this 25-minute time interval. (b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer.
The reaction SO2Cla(g) → SO2(g) + Cla(g) is a first order reaction with a rate constant of 2.2 x 10-5 s-1 at 320 °C. (a) Calculate the half-life for the reaction. (b) What percent of SO2Clz is decomposed after heating the substance at 320°C for 2.0 h?
Sulfonation of benzene has the following mechanism:(a) Write an overall equation for the reaction.(b) Write the overall rate law for the initial rate of the reaction.
Cyclopropane isomerizes to propylene according to a first- order reaction: cyclopropane → propylene The activation energy is E, = 272 kJ mol-1. At 500°C, the reaction rate constant is 6.1 × 10-4 s-1. (a) Calculate the Arrhenius factor A for this reaction. (b) Calculate the rate constant for this reaction at 25°C.