The rate constant k for a certain reaction is measured at two different temperatures:temperature147.0 °C1.8 x 101011216.0 °C 3.2x 10Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction.Round your answer to 2 significant digits.kJE = \|mol

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Description: The rate constant k for a certain reaction is measured at two different temperatures:temperature147.0 °C1.8 x 101011216.0 °C 3.2x 10Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction.Round y

Given-> T1 = 147.0°C = 147.0 + 273 = 420 K T2 = 216.0°C = 216.0 +273 = 489 K K1= 1.8 × 1010 K2=…

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UD OM1 e paunsspau SI Uompau UIPua temperature 147.0 °C 1.8 x 1010 216.0 °C 3.2 x 101 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E 3= ロ。 mol

UD OM1 e paunsspau SI Uompau UIPua temperature 147.0 °C 1.8 x 1010 216.0 °C 3.2 x 101 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E 3= ロ。 mol

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 23P

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