### Thermodynamics of Aluminum Oxide Decomposition**Reaction Equation:**\[ \text{Al}_2\text{O}_3 (s) \rightarrow 2 \text{Al} (s) + \frac{3}{2} \text{O}_2 (g) \]\[ \Delta H_{\text{rxn}} = 1676 \text{ kJ} \]#### Question 1:**Is this reaction endothermic or exothermic?**- [Choose] - 1676 kJ - 440 kJ - endothermic - 1760 kJ - 879 kJ - exothermic #### Question 2:**If 1.049 moles of aluminum were formed by the reaction, how much heat (kJ) would be involved?**---**Explanation:**The provided image contains a chemical reaction where aluminum oxide (\(\text{Al}_2\text{O}_3\)) decomposes into aluminum (\(\text{Al}\)) and oxygen gas (\(\(\text{O}_2)\)). The reaction has an enthalpy change \(\(\Delta H_{\text{rxn}}\)) of 1676 kJ. The nature of the reaction, whether it is endothermic or exothermic, needs to be determined by identifying whether heat is absorbed or released. Additionally, if a specific amount of aluminum is formed, the heat involved in the reaction can be calculated.- **Endothermic Reaction:** Absorbs heat from the surroundings (\(\Delta H > 0\)).- **Exothermic Reaction:** Releases heat to the surroundings (\(\Delta H < 0\)).Given that \(\(\Delta H_{\text{rxn}}\)) is a positive value (1676 kJ), this reaction is endothermic, meaning it absorbs heat.For calculating the heat involved when 1.049 moles of aluminum are formed:- According to the stoichiometric equation, 2 moles of aluminum require 1676 kJ of heat.- For 1.049 moles of aluminum:\[ \text{Heat involved} = \frac{1676 \text{ kJ} }{2} \times 1.049 = 440 \text{ kJ} \]The dropdown menus below each question facilitate user interaction to select the correct answer based on their understanding of

Answered: Image /qna-images/answer/c0deeeea-363c-4f76-abc3-dd33b019ea4c.jpg

(7.6) Aluminum oxide decomposes to aluminum and oxygen gas by the following reaction. Al2O3(s) 2Al(s) + 3/2 O2(g) → A Hrxn = 1676 kJ Is this reaction endothermic or exothermic? [Choose ] [Choose ] 1676 kJ If 1.049 moles of aluminum was formed by the reaction, how much heat (kJ) would be involved? 440 kJ endothermic 1760 kJ 879 kJ exothermic

(7.6) Aluminum oxide decomposes to aluminum and oxygen gas by the following reaction. Al2O3(s) 2Al(s) + 3/2 O2(g) → A Hrxn = 1676 kJ Is this reaction endothermic or exothermic? [Choose ] [Choose ] 1676 kJ If 1.049 moles of aluminum was formed by the reaction, how much heat (kJ) would be involved? 440 kJ endothermic 1760 kJ 879 kJ exothermic

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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