The data in the table give the temperature dependence of the rate constant for the reaction N2O5 (g) → 2 NO2 (g) + 1/2 O2 (g) Plot these data in the appropriate way to derive the activation energy for the reaction. T(K) k(s*) 338 4.87 x 10¬8 328 1.50 x 10-8 318 4.98 x 10¬4 308 1.35 x 10¬4 298 3.46 x 10-8 273 7.87 x 10-7 Activation energy = kJ/mol

The data in the table give the temperature dependence of the rate constant for the reaction N2O5 (g) → 2 NO2 (g) + 1/2 O2 (g) Plot these data in the appropriate way to derive the activation energy for the reaction. T(K) k(s*) 338 4.87 x 10¬8 328 1.50 x 10-8 318 4.98 x 10¬4 308 1.35 x 10¬4 298 3.46 x 10-8 273 7.87 x 10-7 Activation energy = kJ/mol

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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Organic compounds that contain large proportions of nitrogen and oxygen tend to be unstable and are easily decomposed. Hexanitroethane, C2(NO2)6, decomposes according to the equation C2(NO2)6- 2NO, + 4NO + 2CO, The reaction in CCl, solvent is first order with respect to Cz{NO2)s At 63.7°C, k= 0.000254 s* and at 112.6°C, k = 0.0126s*. (a) What is the half-life of C2{NO2); at 63.7 °C? i seconds e Textbook and Media (b) What is the half-life of C2(NO2)s at 112.6 °C? seconds (c) IF0.100 mol of C2(NO2)6 is dissolved in CCI4 at 63.7°C to give 1.00 L of solution, what will be the C2(NO2), concentration after 50.0 minutes? i M (d) What is the value of the activation energy of this reaction, expressed in kilojoules? i kJ/mol (e) What is the rate constant at 159.4 °C?
Determine the activation energy graphically. K(M¹-s¹) T(°C) 1.87×10 600 650 0.0113 0.0569 0.244 700 750
Determine the rate law and the value of k for the following reaction using the data provided. NO,(9) + O3(g) – NO3(g) + O2(g) [NO,li (M) 0.1 0.1 [03li (M) Initial Rate (ms-1) 1 0.33 1.42 2 0.66 2.84 0.25 0.66 7.10 Rate = 43 M's INO,0,] S. -25c O Rate = 1360 M2s"INO,110,] S. Rate = 227 M25s INO,J[0,125 O Rate = 430 M?s INO,10,
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what is the activation energy for a first-order reaction if k = 2.5 x 10-3 s-1 at 332 K and k = 0.15 s-1 at 375 K?
The values of the rate constant for the A→Products reaction are given in the table below with the change of temperature. Find the activation energy for this reaction. k 0.027 0.040 0.059 0.085 0.12 0.17 0.24 t (oC) 1 6 11 16 21 26 31
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Sketch a potential energy diagram for the decomposition of nitrous oxide. N2O(g) →→ N2(g) + O(g) The activation energy for the forward reaction is 171 kJ; If the activation energy for the reverse reaction is 99 kJ, calculate the standard enthalpy change for this reaction. Transfer all the information into an energy diagram. label appropriately
A general reaction written as 2A + 2B → C + 2D is studied and yields the following data. [A]0 [B]0 Initial Δ[C]/Δt 0.100 M 0.100 M 4.00 × 10–5 mol/L • s 0.200 M 0.100 M 4.00 × 10–5 mol/L • s 0.100 M 0.200 M 8.00 × 10–5 mol/L • s What is the overall order of the reaction? Question 8 options: A) 0 B) 2 C) 3 D) 4 E) 1
Using the following reaction: A + 2B → C + D Describe how the rate of disappearance of B will compare to the rate of appearance of C at the start of a reaction. It is determined that A and B are first order reactants. Explain how you would write out the rate law and units of the equilibrium constant with respect to the equation above.
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For a certain reaction, the activation energy is found to be (1.77x10^1) kJ/mol. If the rate constant is (3.6x10^-5) at (3.78x10^2) K, what is the rate constant at (6.290x10^2) K? R = 8.314 J/Kmol; T(K) = T(°C) + 273