The rate of the elementary reactionNO + CH3 OCH3 → HNO + CH3 OCH₂has been studied as a function of temperature between 773 and 873 K. The following data were obtained for the rate constant, k:Temperature (K) k,773793A =813833Lmol s5.37 x 10-²1.10 × 10-¹2.16 × 10-¹4.11 x 10-¹Calculate the activation energy of this reaction.Ea =kJ/molCalculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant.Lmol s

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The rate of the elementary reaction NO + CH3 OCH3 → HNO + CH3 OCH2 has been studied as a function of temperature between 773 and 873 K. The following data were obtained for the rate constant, k: Temperature (K) k, 773 A = 793 813 833 L mol s 5.37 x 10-2 1.10 x 10-¹ 2.16 x 10-1 4.11 x 10-1 Calculate the activation energy of this reaction. Ea = kJ/mol Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. L mol s

The rate of the elementary reaction NO + CH3 OCH3 → HNO + CH3 OCH2 has been studied as a function of temperature between 773 and 873 K. The following data were obtained for the rate constant, k: Temperature (K) k, 773 A = 793 813 833 L mol s 5.37 x 10-2 1.10 x 10-¹ 2.16 x 10-1 4.11 x 10-1 Calculate the activation energy of this reaction. Ea = kJ/mol Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. L mol s

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.35PAE: 11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been...

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