StudentLecture_11

StudentLecture_11 - Lecture 11 10-1-09 Reading for Lecture...

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1 Lecture 11 10-1-09 Reading for Lecture 11: Sections 8.2 (part), pp. 351-353; Section 8.9, pp. 386-392 No Lab next week. Homework due Friday. Reading for Lecture 12: Reading: Sections 8.2 pp 353-356, 8.4, 8.5, pp. 361-367
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2 Energy Content There is a 25% loss in energy when using a mix of 85% ethanol and 15% gasoline (E-85) as compared to 100% gasoline. Why? Ethanol: CH 3 CH 2 OH(l) + 3 O 2 (g) 2 CO 2 (g) + 3 H 2 O(g) ΔH = 30 kj/g Octane, a good approximation to gasoline: C 8 H 18 (l) + 16½ O 2 (g) 8 CO 2 (g) + 9 H 2 O(g) ΔH = 48kj/g On average, the covalent bonds are stronger in ethanol than in octane. Today we will see why that effects the energy available. Density also plays a part e there are more Molecules of ethanol in a liter of ethanol than molecules of octane in a liter of octane.)
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3 Electrostatic attraction and repulsion in covalent in covalent compounds H 1s orbital H 2 covalent bond
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Bond Energy: Energy required to overcome the electrostatic attraction of a bond and separate its components as isolated atoms. Bond Length:
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StudentLecture_11 - Lecture 11 10-1-09 Reading for Lecture...

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