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5. Consider the combustion reaction of octane (C3H18, mol. wt. =114.23 g/mol, density = 0.703 g/mL). a. Write out the balanced chemical equation for this reaction. All products are in the gas phase. b. Calculate the standard free energy (in kJ/mol) released in this reaction. c. Making the approximation that gasoline consists of 100% octane, how much energy would 1.00 gallon of gasoline release? (1 quart = 946 mL, 1 gallon = 4 quarts) AHº (kJ/mol) Sº (J/K mol) Octane(l) -208.4 463.7 H2O(g) -242 189 CO2(g) -393.5 214

5. Consider the combustion reaction of octane (C3H18, mol. wt. =114.23 g/mol, density = 0.703 g/mL). a. Write out the balanced chemical equation for this reaction. All products are in the gas phase. b. Calculate the standard free energy (in kJ/mol) released in this reaction. c. Making the approximation that gasoline consists of 100% octane, how much energy would 1.00 gallon of gasoline release? (1 quart = 946 mL, 1 gallon = 4 quarts) AHº (kJ/mol) Sº (J/K mol) Octane(l) -208.4 463.7 H2O(g) -242 189 CO2(g) -393.5 214

Chemistry
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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Please answer question 5A, 5B, and 5C. 

5. Consider the combustion reaction of octane (C3H18, mol. wt. =114.23 g/mol, density = 0.703 g/mL). a. Write out the balanced chemical equation for this reaction. All products are in the gas phase. b. Calculate the standard free energy (in kJ/mol) released in this reaction. c. Making the approximation that gasoline consists of 100% octane, how much energy would 1.00 gallon of gasoline release? (1 quart = 946 mL, 1 gallon = 4 quarts) AHº (kJ/mol) Sº (J/K mol) Octane(l) -208.4 463.7 H2O(g) -242 189 CO2(g) -393.5 214
Transcribed Image Text:5. Consider the combustion reaction of octane (C3H18, mol. wt. =114.23 g/mol, density = 0.703 g/mL). a. Write out the balanced chemical equation for this reaction. All products are in the gas phase. b. Calculate the standard free energy (in kJ/mol) released in this reaction. c. Making the approximation that gasoline consists of 100% octane, how much energy would 1.00 gallon of gasoline release? (1 quart = 946 mL, 1 gallon = 4 quarts) AHº (kJ/mol) Sº (J/K mol) Octane(l) -208.4 463.7 H2O(g) -242 189 CO2(g) -393.5 214
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