In 2004, New York City Transit started to use ultra-low sulfur kerosene to fuel its fleet of buses. A few years later, the industry standard became ultra-low sulfur diesel. The combustion of these two fuels and of gasoline (assume octane) are represented by the following equations (assuming an average molecular formula of C12H26 for kerosene and an average molecular formula of C12H23 for diesel). Kerosene 2C12H26(1) + 3702(g) → 24CO₂+26H₂O(g) AH = -15743 kJ Diesel 4C12H23(1) + 7102(9)→ 48CO2 + 46H₂O(g) Octane 2C8H18(1) +250₂(g) 16CO₂ + 18H₂O(g) A,H°-10148 kJ The enthalpy change per mole of each fuel is calculated to be Fuel kerosene diesel octane Fuel kerosene Record your answers to one decimal place. Include signs; do not include units. diesel Using your recorded molar enthalpy values from Question 1, calculate the enthalpy change per gram of each fuel. octane Fuel Enthalpy change per mole (kJ/mol) + kerosene + diesel octane ArH=-29989 kJ Record your answer to one decimal place; include signs; do not include units Enthalpy change per gram (kJ/g) ♦ The enthalpy change per mole of carbon dioxide released is calculated to be ♦ Enthalpy change per mol of carbon dioxide released. (kJ/mol) + + Record your answers to 3 significant digits; include signs; do not include units
In 2004, New York City Transit started to use ultra-low sulfur kerosene to fuel its fleet of buses. A few years later, the industry standard became ultra-low sulfur diesel. The combustion of these two fuels and of gasoline (assume octane) are represented by the following equations (assuming an average molecular formula of C12H26 for kerosene and an average molecular formula of C12H23 for diesel). Kerosene 2C12H26(1) + 3702(g) → 24CO₂+26H₂O(g) AH = -15743 kJ Diesel 4C12H23(1) + 7102(9)→ 48CO2 + 46H₂O(g) Octane 2C8H18(1) +250₂(g) 16CO₂ + 18H₂O(g) A,H°-10148 kJ The enthalpy change per mole of each fuel is calculated to be Fuel kerosene diesel octane Fuel kerosene Record your answers to one decimal place. Include signs; do not include units. diesel Using your recorded molar enthalpy values from Question 1, calculate the enthalpy change per gram of each fuel. octane Fuel Enthalpy change per mole (kJ/mol) + kerosene + diesel octane ArH=-29989 kJ Record your answer to one decimal place; include signs; do not include units Enthalpy change per gram (kJ/g) ♦ The enthalpy change per mole of carbon dioxide released is calculated to be ♦ Enthalpy change per mol of carbon dioxide released. (kJ/mol) + + Record your answers to 3 significant digits; include signs; do not include units
General Chemistry - Standalone book (MindTap Course List)
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter3: Calculations With Chemical Formulas And Equaitons
Section: Chapter Questions
Problem 3.141QP: A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume...
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The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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Transcribed Image Text:In 2004, New York City Transit started to use ultra-low sulfur kerosene to fuel its
fleet of buses. A few years later, the industry standard became ultra-low sulfur
diesel. The combustion of these two fuels and of gasoline (assume octane) are
represented by the following equations (assuming an average molecular formula
of C12H26 for kerosene and an average molecular formula of C12H23 for diesel).
Kerosene
2C12H26(1) + 370₂(g) → 24CO₂ + 26H₂O(g) A,H° = -15743 kJ
Diesel
4C12H23(1) + 710₂(g) → 48CO₂ + 46H₂O(g)
Octane
2C8H18(1) +250₂(g) → 16CO₂ + 18H₂O(g) A,H° -10148 kJ
The enthalpy change per mole of each fuel is calculated to be
Fuel
kerosene
diesel
octane
Fuel
kerosene
diesel
Record your answers to one decimal place. Include signs; do not include
units.
octane
Using your recorded molar enthalpy values from Question 1, calculate the
enthalpy change per gram of each fuel.
Fuel
Enthalpy change per mole (kJ/mol)
;
kerosene
+
diesel
+
octane
ΔΙΗ° = -29989 kJ
Enthalpy change per gram (kJ/g)
+
Record your answer to one decimal place; include signs; do not include
units
+
The enthalpy change per mole of carbon dioxide released is calculated to be
+
Enthalpy change per mol of carbon dioxide released
(kJ/mol)
÷
+
Record your answers to 3 significant digits; include signs; do not include
units
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