Understanding the high-temperature behavior of nitrogen oxides is essential for controlling pollution generated in automobile engines. The decomposition of nitric oxide (NO) to N₂and O2 is second order with a rate constant of 0.0797 M-¹.•s-¹ at 735 °C and 0.0816 M-1 -1 at 949 °C.. SPart ACalculate the activation energy for the reaction.Express your answer in kilojoules per mole to three significant figures.► View Available Hint(s)Ea =15. ΑΣΦ?kJ/mol

Check the formula for activation energy and use it to calculate the activation energy.

Understanding the high-temperature behavior of nitrogen oxides is essential for controlling pollution generated in automobile engines. The decomposition of nitric oxide (NO) to N₂ and O₂ is second order with a rate constant of 0.0797 M-1.s¹ at 735 °C and 0.0816 M-1.s-1 at 949 °C. Part A Calculate the activation energy for the reaction. Express your answer in kilojoules per mole to three significant figures. ► View Available Hint(s) Ea = —| ΑΣΦ ? kJ/mol

Understanding the high-temperature behavior of nitrogen oxides is essential for controlling pollution generated in automobile engines. The decomposition of nitric oxide (NO) to N₂ and O₂ is second order with a rate constant of 0.0797 M-1.s¹ at 735 °C and 0.0816 M-1.s-1 at 949 °C. Part A Calculate the activation energy for the reaction. Express your answer in kilojoules per mole to three significant figures. ► View Available Hint(s) Ea = —| ΑΣΦ ? 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...

See similar textbooks

Similar questions

The table shows the variation of the rate constant with temperature for the first-order reaction. 2N₂O5 (g) 2N₂O₂(g) + O₂(g) Determine graphically the activation energy for the reaction. Be sure your answer has the correct number of significant digits. T(K)|*(--) S 298. 1.74 x 10 308. 6.61 × 10 318. 2.52 × 10 328. 7.59 × 10 338. 2.40 × 10 - 5 -5 -4 -4 3 Note: Reference the Fundamental constants table for additional information.
A substance decomposes according to first order kinetics. The rate constants at various temperatures are as follows: T(°C) 600 650 700 750 k (S^(-1)) 1.87x10-3 0.0113 0.569 0.244 Calculate the activation energy required
References] Calculate the activation energy, Ea, for the reaction 2 N₂O5 (g) →4 NO2(g) + O2(g) from the observed rate constants: k at 25 °C 3.46 x 105 s¹ and k at 53 °C 1.20 x 10-3 s¹. The gas constant R is 8.3145 x 10³ kJ/mol. K. = kJ/mol
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 248.0 °C 9.9 x 108 169.0 °C 9.8 x 107 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E = x10 mol X S ?
Determine the activation energy, Ea, (in kJ/mol) of the decomposition reaction, CH3CHO → CH4 + CO. k (M-1/2 s-1) T (°C) 0.01028 940 0.0655 1380
6
The first-order rate constant for the decomposition of N2O5, 2N2O5 (g)→4NO2(g) + O2 (g) Part A at 70° C is 6.82 × 10¬3 s. Suppose we start with 2.60x10-2 mol of N2O5 (g) in a volume of 2.5 L. How many moles of N2O5 will remain after 4.0 min ? Express the amount in moles to two significant digits.
The rate constant for the reaction below at 701K is 2.57 M-1s-1.NO2 (g) + CO (g) → NO (g) + CO (g)Calculate the rate constant at 895K given the activation energy to be 145 kJ/mol.
Enter your answer in the provided box. The variation of the rate constant with temperature for the first-order reaction 2N205(g) 2N204(g) + 02(g) is given in the following table. Determine graphically the activation energy in kJ/mol for the reaction. T(K)k(s1) 298 1.74 x 10-5 308 6.61 x 10-5 318 2.52 x 10 4 328 7.59 x 10 338 2.40 x 103 kJ/mol
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 407.0 °C 4.8 x 10¹0 268.0 °C 2.3 × 10 ¹0 a Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E = x10 a mol X 3 ?
A certain reaction has an activation energy of 68.0 kJ/mol and a frequency factor of A1 = 1.70x1012 M-'s-1 . What is the rate constant, k, of this reaction at 30.0 °C ? Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash.
The rate constants for the decomposition of dinitrogen pentoxide are3.7x10-5 s-1 at 25 oC and 1.7x10-3 s-1 at 55 oC.2 N2O5 (g) → 4 NO2 (g) + O2 (g) -Determine the activation energy for this reaction in KJ/mol.