How much heat, in kJ, is produced by the amount of octane needed to drive 619 kilometers in a car that averages 12.3 km/L?[Blank Text Box] kJ*Explanation: There is no graph or diagram present in the image, only a question followed by a blank text box for an answer.* When octane (C₈H₁₈, density = 0.699 g/mL) undergoes complete combustion, it provides energy according to the reaction:\[ 2 \, \text{C}_8\text{H}_{18}(l) + 25 \, \text{O}_2(g) \rightarrow 16 \, \text{CO}_2(g) + 18 \, \text{H}_2\text{O}(l) \quad \Delta H^{\circ} = -10,932 \, \text{kJ} \]**Explanation:**This chemical equation represents the complete combustion of octane. Two moles of liquid octane react with 25 moles of gaseous oxygen to produce 16 moles of gaseous carbon dioxide and 18 moles of liquid water. The reaction releases energy, indicated by the negative enthalpy change (\(\Delta H^{\circ} = -10,932 \, \text{kJ}\)), signifying that it is an exothermic reaction.

Combustion reaction: 2C8H18(l) + 25O2(g) → 16CO2(g) + 18 H2O(l) Energy released on combustion of 2…

Answered: How much heat, in kJ, is produced by…

How much heat, in kJ, is produced by the amount of octane needed to drive 619 kilometers in a car that averages 12.3 km/L? 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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Question

How much heat, in kJ, is produced by the amount of octane needed to drive 619 kilometers in a car that averages 12.3 km/L?

[Blank Text Box] kJ

*Explanation: There is no graph or diagram present in the image, only a question followed by a blank text box for an answer.*

When octane (C₈H₁₈, density = 0.699 g/mL) undergoes complete combustion, it provides energy according to the reaction:

\[ 2 \, \text{C}_8\text{H}_{18}(l) + 25 \, \text{O}_2(g) \rightarrow 16 \, \text{CO}_2(g) + 18 \, \text{H}_2\text{O}(l) \quad \Delta H^{\circ} = -10,932 \, \text{kJ} \]

**Explanation:**

This chemical equation represents the complete combustion of octane. Two moles of liquid octane react with 25 moles of gaseous oxygen to produce 16 moles of gaseous carbon dioxide and 18 moles of liquid water. The reaction releases energy, indicated by the negative enthalpy change (\(\Delta H^{\circ} = -10,932 \, \text{kJ}\)), signifying that it is an exothermic reaction.

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