**Chemical Reaction and Heat Exchange Analysis** Consider the reaction: \[ 2 \text{Fe}_2\text{O}_3 \rightarrow 4 \text{Fe} + 3 \text{O}_2 \] \[ \Delta H^\circ_{\text{rxn}} = +824.2 \, \text{kJ} \] The decomposition of 79.0 g of Fe₂O₃ results in: - ○ the release of 32600 kJ of heat. - ○ the absorption of 204 kJ of heat. - ○ the release of 204 kJ of heat. - ○ the absorption of 408 kJ of heat. - ○ the absorption of 32600 kJ of heat. - ○ the release of 408 kJ of heat. **Analysis of ΔH (Enthalpy Change):** - The positive ΔH value indicates an endothermic reaction, meaning that the reaction absorbs heat. **Educational Explanation:** - To find the heat change for the decomposition of 79.0 g of Fe₂O₃, the molar mass of Fe₂O₃ should be used to convert the grams to moles. The stoichiometry of the balanced equation and the given ΔH can then be used to determine the heat absorbed or released for this specific mass of Fe₂O₃.

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...
icon
Related questions
Question
**Chemical Reaction and Heat Exchange Analysis**

Consider the reaction:

\[ 2 \text{Fe}_2\text{O}_3 \rightarrow 4 \text{Fe} + 3 \text{O}_2 \]
\[ \Delta H^\circ_{\text{rxn}} = +824.2 \, \text{kJ} \]

The decomposition of 79.0 g of Fe₂O₃ results in:

- ○ the release of 32600 kJ of heat.
- ○ the absorption of 204 kJ of heat.
- ○ the release of 204 kJ of heat.
- ○ the absorption of 408 kJ of heat.
- ○ the absorption of 32600 kJ of heat.
- ○ the release of 408 kJ of heat. 

**Analysis of ΔH (Enthalpy Change):**
- The positive ΔH value indicates an endothermic reaction, meaning that the reaction absorbs heat. 

**Educational Explanation:**
- To find the heat change for the decomposition of 79.0 g of Fe₂O₃, the molar mass of Fe₂O₃ should be used to convert the grams to moles. The stoichiometry of the balanced equation and the given ΔH can then be used to determine the heat absorbed or released for this specific mass of Fe₂O₃.
Transcribed Image Text:**Chemical Reaction and Heat Exchange Analysis** Consider the reaction: \[ 2 \text{Fe}_2\text{O}_3 \rightarrow 4 \text{Fe} + 3 \text{O}_2 \] \[ \Delta H^\circ_{\text{rxn}} = +824.2 \, \text{kJ} \] The decomposition of 79.0 g of Fe₂O₃ results in: - ○ the release of 32600 kJ of heat. - ○ the absorption of 204 kJ of heat. - ○ the release of 204 kJ of heat. - ○ the absorption of 408 kJ of heat. - ○ the absorption of 32600 kJ of heat. - ○ the release of 408 kJ of heat. **Analysis of ΔH (Enthalpy Change):** - The positive ΔH value indicates an endothermic reaction, meaning that the reaction absorbs heat. **Educational Explanation:** - To find the heat change for the decomposition of 79.0 g of Fe₂O₃, the molar mass of Fe₂O₃ should be used to convert the grams to moles. The stoichiometry of the balanced equation and the given ΔH can then be used to determine the heat absorbed or released for this specific mass of Fe₂O₃.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

Blurred answer
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY