Solve both please... Question 18Calculate the activation energy for the reaction (in kJ/mol) when at 618 K the rate constant for thereaction shown below is 0.0000500, and at 216 K the rate constant is 0.00000500.2N,0;(9) → 4NO(9) + 30,(9)01.59025.406.3603.18012.7Question 19Calculate the rate constant (in units 1/M-min) for a second order reaction with a half life of 46.0minutes and an initial concentration of 0.240 M:0.0.04530.27200.1810.03020.0906

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Question 18 Calculate the activation energy for the reaction (in k]/mol) when at 618 K the rate constant for the reaction shown below is 0.0000500, and at 216 K the rate constant is 0.00000500. 2N,0;(9) → 4NO(g) + 30,(g) 01.59 025,4 0636 03.18 012.7 Question 19 Calculate the rate constant (in units 1/M-min) for a second order reaction with a half life of 46.0 minutes and an initial concentration of 0.240 M: 0.0453 00.272 00.181 0.0302 0.0906

Question 18 Calculate the activation energy for the reaction (in k]/mol) when at 618 K the rate constant for the reaction shown below is 0.0000500, and at 216 K the rate constant is 0.00000500. 2N,0;(9) → 4NO(g) + 30,(g) 01.59 025,4 0636 03.18 012.7 Question 19 Calculate the rate constant (in units 1/M-min) for a second order reaction with a half life of 46.0 minutes and an initial concentration of 0.240 M: 0.0453 00.272 00.181 0.0302 0.0906

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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