Hh.195. 2N₂O(g) → 2N,(g) + 0(g)The rate law for the reaction represented above is experimentally determined to be rate kN₂O). Which of the following best explains why increasing the initial concentration of N₂O(g) ataconstant temperature increases the reaction rate?AOODMolecular collisions become more frequentThere is a higher probability of effective molecular collisions.The tate constant for the reaction increases.The reaction mechanism changes to one that has a lower activation energy

The rate law equation expresses the relationship between the rate of a chemical reaction and the…

2N₂O(g) → 2N,(g) + 0,(g) The rate law for the reaction represented above is experimentally determined to be rate kN₂O. Which of the following best explains why increasing the initial concentration of N₂O(g) ata constant temperature increases the reaction rate? A 0 @ Molecular collisions become more frequent There is a higher probability of effective molecular collisions. The tate constant for the reaction increases. D The reaction mechanism changes to one that has a lower activation energy

2N₂O(g) → 2N,(g) + 0,(g) The rate law for the reaction represented above is experimentally determined to be rate kN₂O. Which of the following best explains why increasing the initial concentration of N₂O(g) ata constant temperature increases the reaction rate? A 0 @ Molecular collisions become more frequent There is a higher probability of effective molecular collisions. The tate constant for the reaction increases. D The reaction mechanism changes to one that has a lower activation energy

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.50QE

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