I don’t know how to do this question using the Arrhenius Equation and rate constant. Use the References to access important values if needed for this question.The low pressure pyrolysis of nitroethane takes place according to a first-order reaction:C,H;NO2(g) C¿H4(g) +HNO,(g)The activation energy is Ea = 180 kJ mol"!. At 494°C, the reaction rate constant is 0.313 s-1.(a) Calculate the Arrhenius factor A for this reaction.(b) Calculate the rate constant for this reaction at 394°C.s-1Submit AnswerRetry Entire Group7 more group attempts remainingPreviousNextEmail InstructorSaveCengage Learning | Cengage Technical SupportDIIDDF3F4F5F6F7F8F9F10F11F122$&()+478.Y{}[FGHJK.. .-くoト

Given information, Ea (Activation energy) = 180 kJ/mol = 180*103 J/mol Temperature (T) = 494°C = 494…

The low pressure pyrolysis of nitroethane takes place according to a first-order reaction: C,H;NO2(g) C,H¼(g) +HNO,(g) The activation energy is Ea = 180 kJ mol". At 494°C, the reaction rate constant is 0.313 s. (a) Calculate the Arrhenius factor A for this reaction. (b) Calculate the rate constant for this reaction at 394°C. Submit Answer Retry Entire Group 7 more group attempts remaining

The low pressure pyrolysis of nitroethane takes place according to a first-order reaction: C,H;NO2(g) C,H¼(g) +HNO,(g) The activation energy is Ea = 180 kJ mol". At 494°C, the reaction rate constant is 0.313 s. (a) Calculate the Arrhenius factor A for this reaction. (b) Calculate the rate constant for this reaction at 394°C. Submit Answer Retry Entire Group 7 more group attempts remaining

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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