The reaction between nitrogen dioxide and carbon monoxide is NO₂(g) + CO(g) → NO(g) + CO₂(g) The rate constant at 701 K is measured as 2.57 M-¹.s-¹ and that at 895 K is measured as 567 M-¹.s-¹. ▼ Part A Use the value of the activation energy (E₁ = 1.50 x 10² kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 457 K. k= ΠΙ ΑΣΦ 6 ? M-1.8-1
The reaction between nitrogen dioxide and carbon monoxide is NO₂(g) + CO(g) → NO(g) + CO₂(g) The rate constant at 701 K is measured as 2.57 M-¹.s-¹ and that at 895 K is measured as 567 M-¹.s-¹. ▼ Part A Use the value of the activation energy (E₁ = 1.50 x 10² kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 457 K. k= ΠΙ ΑΣΦ 6 ? M-1.8-1
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
Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 108CWP: Consider the hypothetical reaction A2(g) + B2(g) 2AB(g), where the rate law is: [A2]t=k[A2][B2] The...
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