Please use the values in the resources listed below instead of the textbook values. The rate of the electron-exchange reaction between naphthalene (C10H8) and its anion radical (C10H8¬) in an organic solvent is diffusion controlled. C10H8¯ + C10H8 =C10H8 + C10H8¯ The reaction is bimolecular and second order. The rate constants are as follows. T/K 305 295 291 275 k/109 M-1.s-1 2.64 2.21 2.05 1.49 Calculate the values of Ea, AH°t, ASof and AGot at 295 K for the reaction. [Hint: Rearrange the equation below and plot In(k/T) versus 1/T.] KBT T easot/Re-AHot/RT(M1 – m) k = Ea = 2993.386 x kJ-mol-1 X kJ-mol-1 x J-K-1.mol-1 AH°† = 2991.1 ASo# = -28069.52 AG°† = 107010.2 X kJ•mol-1

Please use the values in the resources listed below instead of the textbook values. The rate of the electron-exchange reaction between naphthalene (C10H8) and its anion radical (C10H8¬) in an organic solvent is diffusion controlled. C10H8¯ + C10H8 =C10H8 + C10H8¯ The reaction is bimolecular and second order. The rate constants are as follows. T/K 305 295 291 275 k/109 M-1.s-1 2.64 2.21 2.05 1.49 Calculate the values of Ea, AH°t, ASof and AGot at 295 K for the reaction. [Hint: Rearrange the equation below and plot In(k/T) versus 1/T.] KBT T easot/Re-AHot/RT(M1 – m) k = Ea = 2993.386 x kJ-mol-1 X kJ-mol-1 x J-K-1.mol-1 AH°† = 2991.1 ASo# = -28069.52 AG°† = 107010.2 X kJ•mol-1

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

Please show your work (THIS IS NOT A GRADED ASSIGNMENT)
The vapor phase dimerization of trifluorochloroethylene to 1,2-dichloro-1,2,3,3,4,4-hexafluorocyclobutane takes place according to a second-order reaction: 2C₂CIF3(g) C₂Cl₂F6(g) The activation energy is Ea = 110 kJ mol-¹. At 507°C, the reaction rate constant is 1.49 L mol¹ s¹1. (a) Calculate the Arrhenius factor A for this reaction. (b) Calculate the rate constant for this reaction at 310°C. mol-1 s-1 L mol-¹ s-1
Part A What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: A+ B Step 2: B+OC →. D (slow) = C (fast) Express your answer in terms of k and the necessary concentrations (e.g., k* [A]^3* [D]). • View Available Hint(s) ΑΣφ rate = Submit
Using the mechanism provided, determine a possible rate law for the following overall reaction: Q2 + 2 AJ2 → 2AJ2Q Step #1. AJ2 + Q2 → AJ2Q + Q slow Step #2. Q + AJ2 → AJ2Q quick Group of answer choices Rate = k [AJ2]2 [Q2] Rate = k [AJ2Q]2 Rate = k [AJ2] [Q] Rate = k [AJ2Q] [Q]2 Rate = k [AJ2] [Q2]
Please show your work (this is not a graded assignment)
The activation energy for the gas phase decomposition of 2-bromopropane is 212 kJ.CH3CHBrCH3CH3CH=CH2 + HBrThe rate constant at 672 K is 3.16×10-4 /s. The rate constant will be 3.76×10-3 /s at K.
If the y-axis of the graph changes to “volume of hydrogen / cm3 ”, sketch this rate curve. What will be the effect on the reaction rate if the concentration of HCl changes from 0.1 M to 0.2 M? Explain
What is the solution concentration after 58 minutes if it was originally 0.14 M H2O2? Round your answer to the nearest 10th of a minute.
I Review | Constants | Period MISSED THIS? Read Section 15.4 (Pages 642 - 649); Watch KCV 15.4, IWVE 15.4.The decomposition of SO2 Cl2 is first order in SO2 Cl2 and has a rate constant of 1.40x104s-1 at a certain temperature. -kt + In(SO2C2]o - (1.40 x 10-s)(220 s) + In 0.175 M In[SO2 Cl2]t %3D -1.774 Take the inverse natural logarithm of both sides of the equation. [SO2 Cl2]: e-1.774 M 0.170 M Part E If the initial concentration of SO2 Cl2 is 0.175 M, what is the concentration of SO2 Cl2 after 510 s ? Express your answer using three significant figures. ΑΣφ (SO2 Cl2]e = M