plz help me with these two questions Using first- and second-order integrated rate lawsConsider this reaction:2NH₂ (g) → N₂ (g) + 3H₂(g)2At a certain temperature it obeys this rate law.rate = (3.71 s¯¹)[NH3]Suppose a vessel contains NH3 at a concentration of 1.38M. Calculate how long it takes for the concentration of NH3 to decrease by 90.0%. You may assumeno other reaction is important.Round your answer to 2 significant digits.Sx10×0/5SIzabe Using the Arrhenius equation to calculate k at one temperature from k at...The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E = 12.0 kJ/mol. If the rate constant of thisareaction is 2.8 × 106 MRound your answer to 2 significant digits.1k = M²¯ ¹- 1 - 1*S−1• Sat 132.0 °C, what will the rate constant be at 47.0 °C?x10XŚ

it is given thatsince the order of the reaction is missing, so we will find the reaction order with…

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E = 12.0 kJ/mol. If the rate constant of this -1 -1 reaction is 2.8 x 106 M 'S Round your answer to 2 significant digits. -1 -1 k = - M •S at 132.0 °C, what will the rate constant be at 47.0 °C? X S

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E = 12.0 kJ/mol. If the rate constant of this -1 -1 reaction is 2.8 x 106 M 'S Round your answer to 2 significant digits. -1 -1 k = - M •S at 132.0 °C, what will the rate constant be at 47.0 °C? X S

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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