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NASA Guide to Engines

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NASA Guide to Engines ( nasa-guide-engines )

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INSTRUCTIONAL OBJECTIVES Students will • Recognize that heat of reaction are additive • Evaluate energy available in different compounds • Recognize the need for oxygen in combustion NATIONAL SCIENCE CONTENT STANDARD B Chemical reactions • Chemical reactions may release or consume energy. Some reactions, such as burning fossil fuels, release large amounts of energy by giving off heat and emitting light. INTRODUCTION Hess’s Law states that enthalpy changes (ΔH) are additive. This means that the sum of the heats of formation of the products minus the sum of the heats of formation of the reactants (each multiplied by their respective coef- ficients in a chemical reaction) will equal the ΔH for the overall reaction. DH = ∑ DHo − ∑ DHo . ( f products ) ( f reactants ) One must first balance the chemical equation and then find the value of ΔHof for each component. Example Problem: When hydrocarbon fuels are burned in an engine, oxygen (O2) is a reactant and carbon dioxide (CO2) and water (H2O) are products. When grilling in the backyard with propane, the equation is C3H8+O2 → CO2+H2O Standard heats of formation in kilocalories per mole (kcal/mol) are C3H8 = –25.0 O2 = 0 CO2 = –94.0 H2O = –68.3 Balance the equation C3H8 + 5 O2 → 3 CO2 + 4 H2O Solution: For each product, multiply the heat of reaction by its reaction coefficient and add them together. Do the same for the reactants. Then take the sum of the heats of formation of the products and subtract the sum of the heats of formation of the reactants to find the overall heat of reaction: DH = [3 (–94.0) + 4 (–68.3)] – [(25.0) + 5 (0.0)] = –530.2 kcal Hess’s Law Pushing the Envelope: A NASA Guide to Engines 37 CHEMISTRY

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