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A(g) B(g) C(g) The rate law for the above reaction is: -d[A]/dt = k[A][B] The rate constant is 3.13x102 L molls1 at 350.o°C and 4.53x104 L mol s at 544.0°C. Use the Arrhenius equation k = Ae E/RT to: Calculate E, for this reaction. 385 kJ/mol Submit Answer Incorrect. Tries 2/99 Previous Tries Calculate the rate constant k at 423.0°C for this reaction. 3.08e-3 M s s-1 Submit Answer Incompatible units. No conversion found between "M*s*s-1" and the required units. Calculate the pre-exponential factor A for this reaction. Submit Answer Tries 0/99

A(g) B(g) C(g) The rate law for the above reaction is: -d[A]/dt = k[A][B] The rate constant is 3.13x102 L molls1 at 350.o°C and 4.53x104 L mol s at 544.0°C. Use the Arrhenius equation k = Ae E/RT to: Calculate E, for this reaction. 385 kJ/mol Submit Answer Incorrect. Tries 2/99 Previous Tries Calculate the rate constant k at 423.0°C for this reaction. 3.08e-3 M s s-1 Submit Answer Incompatible units. No conversion found between "M*s*s-1" and the required units. Calculate the pre-exponential factor A for this reaction. Submit Answer Tries 0/99

Chemistry
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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(Arrhenius equation); I’m not sure what the molecular collision constant (A) would be
A(g) + B(g) C(g) The rate law for the above reaction is: -d[A]/dt = k[A]B] The rate constant is 3.13x102 L mol s at 350.0°C and 4.53×104 L mol s at 544.0°C. Use the Arrhenius equation k = Ae F/RT to: Calculate E- for this reaction. 385 kJ/mol Submit Answer Incorrect. Tries 2/99 Previous Tries Calculate the rate constant k at 423.0°C for this reaction. 3.08e-3 M s^s-1 Submit Answer Incompatible units. No conversion found between "M*s^s-1" and the required units. Calculate the pre-exponential factor A for this reaction. Submit Answer Tries 0/99
Transcribed Image Text:A(g) + B(g) C(g) The rate law for the above reaction is: -d[A]/dt = k[A]B] The rate constant is 3.13x102 L mol s at 350.0°C and 4.53×104 L mol s at 544.0°C. Use the Arrhenius equation k = Ae F/RT to: Calculate E- for this reaction. 385 kJ/mol Submit Answer Incorrect. Tries 2/99 Previous Tries Calculate the rate constant k at 423.0°C for this reaction. 3.08e-3 M s^s-1 Submit Answer Incompatible units. No conversion found between "M*s^s-1" and the required units. Calculate the pre-exponential factor A for this reaction. Submit Answer Tries 0/99
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