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he rate of the elementary reaction NO + Cl₂ → NOCI + Cl as been studied as a function of temperature between 523 and 673 K. The following data were obtained for the rate constant, k: L mol s 1.32 × 10¹ 3.80 x 10¹ 9.83 × 10¹ 2.32 × 10² Temperature (K) k, 523 a = 553 583 613 alculate the activation energy of this reaction. kJ/mol alculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. L mol.s

he rate of the elementary reaction NO + Cl₂ → NOCI + Cl as been studied as a function of temperature between 523 and 673 K. The following data were obtained for the rate constant, k: L mol s 1.32 × 10¹ 3.80 x 10¹ 9.83 × 10¹ 2.32 × 10² Temperature (K) k, 523 a = 553 583 613 alculate the activation energy of this reaction. kJ/mol alculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. L mol.s

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Chemistry
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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
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The rate of the elementary reaction NO + Cl₂ → NOCI + Cl has been studied as a function of temperature between 523 and 673 K. The following data were obtained for the rate constant, k: L mol.s 1.32 × 10¹ 3.80 × 10¹ Temperature (K) k, 523 553 A = 583 613 9.83 × 10¹ 2.32 × 10² 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
Transcribed Image Text:The rate of the elementary reaction NO + Cl₂ → NOCI + Cl has been studied as a function of temperature between 523 and 673 K. The following data were obtained for the rate constant, k: L mol.s 1.32 × 10¹ 3.80 × 10¹ Temperature (K) k, 523 553 A = 583 613 9.83 × 10¹ 2.32 × 10² 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
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