### Thermochemical Reaction Analysis**Reaction:**\[ 4\text{Al}(s) + 3\text{O}_2(g) \rightarrow 2\text{Al}_2\text{O}_3(s) \]**Enthalpy Change:**\[ \Delta H^\circ_{\text{rxn}} = -3351.4 \, \text{kJ} \]**Question:**How much energy is transferred when 15.5 g of \(\text{Al}_2\text{O}_3\) is produced?**Options:**- \(-51,900 \, \text{kJ}\)- \(-3350 \, \text{kJ}\)- \(-1430 \, \text{kJ}\) (Correct)- \(-509 \, \text{kJ}\)- \(-255 \, \text{kJ}\)### ExplanationThe text presents a thermochemical equation indicating that the formation of 2 moles of \(\text{Al}_2\text{O}_3\) from aluminum and oxygen releases \(3351.4 \, \text{kJ}\) of energy. The problem asks to calculate the energy transfer when only 15.5 g of \(\text{Al}_2\text{O}_3\) is produced, as opposed to 2 moles. The correct answer based on this calculation is \(-1430 \, \text{kJ}\).

We can solve the problem by determining the moles of aluminium oxide produced. Data given : ∆H0 = -…

Answered: 4Al(s) + 302(g)- - 2AI2O3(s) AH°rxn =…

4Al(s) + 302(g)- - 2AI2O3(s) AH°rxn = -3351.4 kJ How much energy is transferred when 15.5 g of Al2O3 is produced? -51,900 kJ -3350 kJ O -1430 kJ -509 kJ -255 kJ

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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