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Chemistry > SOLUTIONS MANUAL > University of MichiganCHEM 230230_W16_PREP_E1_key (All)

University of MichiganCHEM 230230_W16_PREP_E1_key

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CHEM 230_F15_E1_PREP p 1 € 12 Br 2(l ) →Br(g) ΔH =111.87 kJ Br 2(l) →Br2(g ) ΔH = 30.91 kJ € 2Br (g) →Br2(l) ΔH = -2(111.87kJ) Br 2(l) →Br2(g ) ΔH = 30.91 kJ € ... 2Br (g) →Br2(g) ΔH = - 223.75 kJ +30.91 kJ = -192.83kJ 1) Find the bond enthalpy of an Br-Br bond given ΔHof Br(g) = 111.87 kJ and ΔHofBr2(g) = 30.9 kJ Bond enthalpy Br-Br : 192.8 kJ/mol 10 5 points for bond enthalpy equation 2) Use the van der Waals constants shown in the table below to answer questions a-d. van der Waals constant a (bar/L2 mol2) b (L/mol) HCl 3.700 0.04061 a) Which is the more polar bond? (Circle one:) N-H or N-F HBr 4.500 0.04415 NH3 4.225 0.03713 NF3 3.58 0.05453 b) In which bond is N the negative end of the dipole? (Circle one): N-H N-F both neither c) Which gas has the lower Z (compression factor) at 10 atm? (Circle one): HCl HBr HCl and HBr have the same Z d) Which gas has the lower Z (compression factor) at 1000 atm? (Circle one): HCl HBr HCl and HBr have the same Z [Show More]

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