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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: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 11.ACP: (Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a...
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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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