HCl reacts with CH3CHCH2 in the gas phase according to the following chemical equation: HC(g) +CH;CHCH2(g) → CH;CHCICH3(g) It is observed that, when the concentration of CH3CHCH, is reduced to 1/2 of its initial value, the rate of the reaction is also reduced to 1/2 of its initial value. When the concentration of HCl is multiplied by 4.18, the rate of the reaction increases by a factor of 73.0. (a) Write the rate expression for this reaction, and give the units of the rate constant k, assuming concentration is expressed as M and time is in seconds. rate = k units = (b) If [HC1] were multiplied by 4.06 and [CH3CHCH2] by 3.98, what change in the rate would be observed? The rate would increase by a factor of |

HCl reacts with CH3CHCH2 in the gas phase according to the following chemical equation: HC(g) +CH;CHCH2(g) → CH;CHCICH3(g) It is observed that, when the concentration of CH3CHCH, is reduced to 1/2 of its initial value, the rate of the reaction is also reduced to 1/2 of its initial value. When the concentration of HCl is multiplied by 4.18, the rate of the reaction increases by a factor of 73.0. (a) Write the rate expression for this reaction, and give the units of the rate constant k, assuming concentration is expressed as M and time is in seconds. rate = k units = (b) If [HC1] were multiplied by 4.06 and [CH3CHCH2] by 3.98, what change in the rate would be observed? The rate would increase by a factor of |

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 5P

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