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The variation of the rate constant with temperature for the decomposition of HI(g) to H2(g) and 12(g) is given below. Use Arrhenius equation to determine the activation energy of the reaction. 2HI(g) H2(g) + 12(9) T (K) K (L/mol/s) 555 3.52 x 10-7 575 1.22 x 10 6 645 8.59 x 10-5 700 1.16 x 10-3 781 95. x 10-2 O Activation energy, E, = 1.65 x 105 J/mol Activation energy, E = 2.65 x 10° J/mol O Activation energy, E, = 3.65 x 10 J/mol O Activation energy, E = 4.65 x 10 J/mol

The variation of the rate constant with temperature for the decomposition of HI(g) to H2(g) and 12(g) is given below. Use Arrhenius equation to determine the activation energy of the reaction. 2HI(g) H2(g) + 12(9) T (K) K (L/mol/s) 555 3.52 x 10-7 575 1.22 x 10 6 645 8.59 x 10-5 700 1.16 x 10-3 781 95. x 10-2 O Activation energy, E, = 1.65 x 105 J/mol Activation energy, E = 2.65 x 10° J/mol O Activation energy, E, = 3.65 x 10 J/mol O Activation energy, E = 4.65 x 10 J/mol

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 60E: The rate constant for the decomposition of acetaldehyde, CH3CHO, t0 methane, CH4, and carbon...
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The variation of the rate constant with temperature for the decomposition of HI(g) to H2(g) and 12(g) is given below. Use Arrhenius equation to determine the activation energy of the reaction. 2HI(g) H2(g) + 12(9) T (K) K (L/mol/s) 555 3.52 x 10-7 575 1.22 x 10-6 645 8.59 x 10-5 700 1.16 x 10-3 781 95. x 10-2 O Activation energy, E, = 1.65 x 10 J/mol O Activation energy, E, = 2.65 x 10° J/mol O Activation energy, E, = 3.65 x 10 J/mol O Activation energy, E = 4.65 x 10 J/mol O O
Transcribed Image Text:The variation of the rate constant with temperature for the decomposition of HI(g) to H2(g) and 12(g) is given below. Use Arrhenius equation to determine the activation energy of the reaction. 2HI(g) H2(g) + 12(9) T (K) K (L/mol/s) 555 3.52 x 10-7 575 1.22 x 10-6 645 8.59 x 10-5 700 1.16 x 10-3 781 95. x 10-2 O Activation energy, E, = 1.65 x 10 J/mol O Activation energy, E, = 2.65 x 10° J/mol O Activation energy, E, = 3.65 x 10 J/mol O Activation energy, E = 4.65 x 10 J/mol O O
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