Given the standard molar enthalpy of formation of hexane is -167.2 kj/mol, determine the C-C bond dissociation energy of cyclohexane.need energy for BDE(C-C) and its standard deviationunit kJ/mol 1) When a mass, m, of cyclohexane is burnt in a constant volume bomb calorimeter with heat capacity Ceal the temperature ofthe water surrounding the calorimeter is raised by AT- The heat of combustion of the nichrome wire used to ignite thereactive mixture is q. The lengths of the nichrome wire before and after combustion are L, and L, respectively. The combustionreaction is carried out at temerature T and pressure P. The standard molar enthalpy of combustion of cyclohexane is written asAH°.Table 1: Experimental conditions and thermodynamic data forthe combustion in the bomb calorimeterA HomCcalqLoLTP-3951 +/-19 kJ/mol0.78 +0.002 g8222.0+/8.0 J/k-9.6 J/cm9. 39 +0.05 cm3. 39 +/-0.05 cm20.65 +/-0.04 C25.8 +/-1.0 bar

The bond dissociation energy (BDE) for cyclohexane involves understanding the bonds that must be…

Answered: 1) When a mass, m, of cyclohexane is…

EBK A SMALL SCALE APPROACH TO ORGANIC L

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ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter26: Biodiesel

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Given the standard molar enthalpy of formation of hexane is -167.2 kj/mol, determine the C-C bond dissociation energy of cyclohexane.
need energy for BDE(C-C) and its standard deviation
unit kJ/mol

1) When a mass, m, of cyclohexane is burnt in a constant volume bomb calorimeter with heat capacity Ceal the temperature of
the water surrounding the calorimeter is raised by AT- The heat of combustion of the nichrome wire used to ignite the
reactive mixture is q. The lengths of the nichrome wire before and after combustion are L, and L, respectively. The combustion
reaction is carried out at temerature T and pressure P. The standard molar enthalpy of combustion of cyclohexane is written as
AH°.
Table 1: Experimental conditions and thermodynamic data for
the combustion in the bomb calorimeter
A Ho
m
Ccal
q
Lo
L
T
P
-3951 +/-19 kJ/mol
0.78 +0.002 g
8222.0+/8.0 J/k
-9.6 J/cm
9. 39 +0.05 cm
3. 39 +/-0.05 cm
20.65 +/-0.04 C
25.8 +/-1.0 bar

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

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