### Understanding Standard Heat of Formation and Reaction EnthalpyThe standard heat of formation, \( \Delta H_f^\circ \), is defined as the enthalpy change for the formation of one mole of a substance from its constituent elements in their standard states. By definition, elements in their standard states have \( \Delta H_f^\circ = 0 \). These formation values are crucial for calculating the enthalpy change of any reaction.#### Calculation ExampleConsider the following reaction:\[ 2 \text{NO} (g) + \text{O}_2 (g) \rightarrow 2 \text{NO}_2 (g) \]Using the heat of formation values from the table below:| Substance | \( \Delta H_f^\circ \) (kJ/mol) ||-----------|--------------------------------|| NO (g) | 90.2 || O2 (g) | 0 || NO2 (g) | 33.2 |The standard heat of reaction (\( \Delta H_{rxn}^\circ \)) for the overall reaction is calculated as follows:\[ \Delta H_{rxn}^\circ = \left( \sum \Delta H_f^\circ \text{(products)} \right) - \left( \sum \Delta H_f^\circ \text{(reactants)} \right) \]\[ \Delta H_{rxn}^\circ = [2(33.2)] - [2(90.2) + 0] \]\[ \Delta H_{rxn}^\circ = 66.4 - 180.4 \]\[ \Delta H_{rxn}^\circ = -114 \text{ kJ} \]### Practice Problem**Part B: Combustion of Heptane**The combustion of heptane (\( \text{C}_7\text{H}_{16} \)) is described by the following reaction:\[ \text{C}_7\text{H}_{16} (g) + 11 \text{O}_2 (g) \rightarrow 7 \text{CO}_2 (g) + 8 \text{H}_2\text{O} (g) \]Given the heat of formation values from the table below:| Substance | \( \Delta H_f^\circ \) (kJ/mol

Combustion Reaction :- For organic compounds in presence of oxygen, they oxidised and forms carbon…

The combustion of heptane, C,H16, occurs via the reaction C;H16(g) + 1102(g)→7CO2(g) + 8H20(g) with heat of formation values given by the following table: AH (kJ/mol) Substance CH16 (g) -187.9 CO2(g) -393.5 H20(g) -241.8 Calculate the enthalpy for the combustion of 1 mole of heptane. Express your answer to four significant figures and include the appropriate units. > View Available Hint(s) ΔΗ Value Units Submit

The combustion of heptane, C,H16, occurs via the reaction C;H16(g) + 1102(g)→7CO2(g) + 8H20(g) with heat of formation values given by the following table: AH (kJ/mol) Substance CH16 (g) -187.9 CO2(g) -393.5 H20(g) -241.8 Calculate the enthalpy for the combustion of 1 mole of heptane. Express your answer to four significant figures and include the appropriate units. > View Available Hint(s) ΔΗ Value Units Submit

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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