steps.TheuvelanUnumber of enzyme-catalyzedisC6H1206 (s) → 2C2H3OH(I) + 2CO2(g)Calculate the standard enthalpy change for this reac-tion, assuming that the carbohydrate is a-D-glucose.Bond Enthalpy3.58 (a) Explain why the bond enthalpy of a moleculeis always defined in terms of a gas-phase reaction.(b) The bond dissociation enthalpy of F2 is 150.6 kJmol-1. Calculate the value of ArHo for F(g)3.59 From the molar enthalpy of vaporization of waterat 373 K and the bond dissociation enthalpies of H2and O2 (see Table 3.4), calculate the average O-H bondenthalpy in water, given thatH2(0) +02(9) H2Ou)285.8 kJ mol-13.60 Use the bond enthalpy values in Table 3.4 to cal-culate the enthalpy of combustion for ethane,2C2H6(g) + 702 (g) → 4CO2(g) + 6H20(1)Compare your result with that calculated from thenthalpy of formation values of the products and reac-ants listed in Appendix 2.

Question
Asked Jan 25, 2019

3.58

steps.
The
uvelan
U
number of enzyme-catalyzed
is
C6H1206 (s) → 2C2H3OH(I) + 2CO2(g)
Calculate the standard enthalpy change for this reac-
tion, assuming that the carbohydrate is a-D-glucose.
Bond Enthalpy
3.58 (a) Explain why the bond enthalpy of a molecule
is always defined in terms of a gas-phase reaction.
(b) The bond dissociation enthalpy of F2 is 150.6 kJ
mol-1. Calculate the value of ArHo for F(g)
3.59 From the molar enthalpy of vaporization of water
at 373 K and the bond dissociation enthalpies of H2
and O2 (see Table 3.4), calculate the average O-H bond
enthalpy in water, given that
H2(0) +02(9) H2Ou)
285.8 kJ mol-1
3.60 Use the bond enthalpy values in Table 3.4 to cal-
culate the enthalpy of combustion for ethane,
2C2H6(g) + 702 (g) → 4CO2(g) + 6H20(1)
Compare your result with that calculated from the
nthalpy of formation values of the products and reac-
ants listed in Appendix 2.
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steps. The uvelan U number of enzyme-catalyzed is C6H1206 (s) → 2C2H3OH(I) + 2CO2(g) Calculate the standard enthalpy change for this reac- tion, assuming that the carbohydrate is a-D-glucose. Bond Enthalpy 3.58 (a) Explain why the bond enthalpy of a molecule is always defined in terms of a gas-phase reaction. (b) The bond dissociation enthalpy of F2 is 150.6 kJ mol-1. Calculate the value of ArHo for F(g) 3.59 From the molar enthalpy of vaporization of water at 373 K and the bond dissociation enthalpies of H2 and O2 (see Table 3.4), calculate the average O-H bond enthalpy in water, given that H2(0) +02(9) H2Ou) 285.8 kJ mol-1 3.60 Use the bond enthalpy values in Table 3.4 to cal- culate the enthalpy of combustion for ethane, 2C2H6(g) + 702 (g) → 4CO2(g) + 6H20(1) Compare your result with that calculated from the nthalpy of formation values of the products and reac- ants listed in Appendix 2.

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check_circleExpert Solution
Step 1

a) Bond enthalpy of a molecule is defined in terms of a gas-phase reaction. This is because in gas-phase, the interactions are negligible. In liquid and solid phase, the molecules have interactions.

Step 2

b) Fluorine molecule has one F-F bond.

Fluorine molecule dissociates to give two fluorine atoms.

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Step 3

Thus, the enthalpy of formation of fluo...

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