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Which element is reduced in this reaction? Justify your answer in terms of the oxidation numbers.

Which element is reduced in this reaction? Justify your answer in terms of the oxidation numbers.

Chemistry
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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please use equation to answer question.

(b) Which element is reduced in this reaction? Justify your answer in terms of the oxidation numbers.
Transcribed Image Text:(b) Which element is reduced in this reaction? Justify your answer in terms of the oxidation numbers.
Equimolar amounts of \( \text{H}_2 \, (g) \) and \( \text{Br}_2 \, (g) \) are injected into an evacuated, rigid container, where they react according to the equation below. \[ \text{H}_2 \, (g) + \text{Br}_2 \, (g) \rightleftharpoons 2 \, \text{HBr} \, (g) \] \[ \Delta H^\circ_{\text{rxn}} = -72.4 \, \text{kJ/mol}_{\text{rxn}} \] This reaction represents the formation of hydrogen bromide (\(\text{HBr}\)) from hydrogen gas (\(\text{H}_2\)) and bromine gas (\(\text{Br}_2\)). The enthalpy change (\(\Delta H^\circ_{\text{rxn}}\)) indicates that the reaction is exothermic, releasing 72.4 kJ of energy per mole of reaction.
Transcribed Image Text:Equimolar amounts of \( \text{H}_2 \, (g) \) and \( \text{Br}_2 \, (g) \) are injected into an evacuated, rigid container, where they react according to the equation below. \[ \text{H}_2 \, (g) + \text{Br}_2 \, (g) \rightleftharpoons 2 \, \text{HBr} \, (g) \] \[ \Delta H^\circ_{\text{rxn}} = -72.4 \, \text{kJ/mol}_{\text{rxn}} \] This reaction represents the formation of hydrogen bromide (\(\text{HBr}\)) from hydrogen gas (\(\text{H}_2\)) and bromine gas (\(\text{Br}_2\)). The enthalpy change (\(\Delta H^\circ_{\text{rxn}}\)) indicates that the reaction is exothermic, releasing 72.4 kJ of energy per mole of reaction.
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