CHEM163B_HW4_solutions_2011

CHEM163B_HW4_solutions_2011 - C bond enthalpy [correctly]...

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Winter 2011 Chemistry 163B Homework #4 Problems (#20-#22) 20. (!Hº f ) 298 for cyclopropane, C 3 H 6 (g) , is 53.30 kJ/mol. a. Use this value of (!Hº f ) 298 to calculate the C ± C bond enthalpy for the carbon- carbon bonds in cyclopropane. Assume standard H ± H and C ± H bond enthalpies of 436 kJ/mole and 413 kJ/mole, respectively, and a !H sublimation of 717 kJ/mole for C(gr) . b. Tables of bond enthalpies (values averaged over a number of hydrocarbons) give a standard C ± C bond enthalpy of 348 kJ/mol. Why does the C
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Unformatted text preview: C bond enthalpy [correctly] calculated in part (a) differ from this standard value? c. Would the experimental value of 53.30 kJ/mol be larger or smaller than (!H f ) 298 calculated using standard bond enthalpies? 21. E&R P4.17d (d only) 22. E&R P5.2 the comment about subtracting an additional 5% implies that an additional factor of 95% efficiency must be included in the overall computation also (note [watt] = [J s-1 ]; 1 watt = 3600 J hr-1 ) 1 413 413 309 309...
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CHEM163B_HW4_solutions_2011 - C bond enthalpy [correctly]...

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