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Consider the reaction Br₂ + H₂➡➡➡ 2HBr The bond dissociation energies are 194 kJ/mol for Br₂, 436 kJ/mol for H₂ and 366 kJ/mol for HBr. Assume the reaction takes place by first breaking the Br₂ and H₂ bonds to make separate atoms. Estimate the activation energy from the bond dissociation energies.

Consider the reaction Br₂ + H₂➡➡➡ 2HBr The bond dissociation energies are 194 kJ/mol for Br₂, 436 kJ/mol for H₂ and 366 kJ/mol for HBr. Assume the reaction takes place by first breaking the Br₂ and H₂ bonds to make separate atoms. Estimate the activation energy from the bond dissociation energies.

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Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Consider the reaction Br₂ + H₂ = 2HBr The bond dissociation energies are 194 kJ/mol for Br₂, 436 kJ/mol for H₂ and 366 kJ/mol for HBr. Assume the reaction takes place by first breaking the Br₂ and H₂ bonds to make separate atoms. Estimate the activation energy from the bond dissociation energies. Energy Plus or minus 2% Br₂ + H₂ kJ/mol 2 Attempts Submit 2HBr
Transcribed Image Text:Consider the reaction Br₂ + H₂ = 2HBr The bond dissociation energies are 194 kJ/mol for Br₂, 436 kJ/mol for H₂ and 366 kJ/mol for HBr. Assume the reaction takes place by first breaking the Br₂ and H₂ bonds to make separate atoms. Estimate the activation energy from the bond dissociation energies. Energy Plus or minus 2% Br₂ + H₂ kJ/mol 2 Attempts Submit 2HBr
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