**Question 6 of 35**In the following reaction, how much heat (in kJ) is released when 2.49 moles of CH₄ are burned?\[ \text{CH}_4 (g) + 2 \, \text{O}_2 (g) \rightarrow \text{CO}_2 (g) + 2 \, \text{H}_2\text{O}(g) \]\[\Delta H^\circ = -802 \, \text{kJ/mol}\]---**Explanation:**This question involves calculating the heat released during the combustion of methane (\(\text{CH}_4\)). The chemical equation provided shows the complete combustion of methane with oxygen (\( \text{O}_2 \)) to form carbon dioxide (\(\text{CO}_2\)) and water vapor (\(\text{H}_2\text{O}\)).The enthalpy change (\(\Delta H^\circ\)) for the reaction is -802 kJ/mol, meaning that 802 kJ of heat is released for every mole of methane burned.To find the total heat released for 2.49 moles of \(\text{CH}_4\):\[ \text{Total Heat Released} = 2.49 \, \text{moles} \times (-802 \, \text{kJ/mol}) \]This calculation will give the total heat energy released in kilojoules (kJ).**Note:** Negative \(\Delta H^\circ\) indicates that the reaction is exothermic, as it releases heat.

given, CH4(g) + 2O2(g) → CO2 (g) + 2 H2O(g) △H= -802 kJ/mol one mole of methane gives 802 kJ of…

Answered: In the following reaction, how much…

In the following reaction, how much heat (in kJ) is released when 2.49 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H;O(g) AH° = -802 %3D kJ/mol

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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