Ethanol can be made by the reaction of ethylene and water: H 2 C=CH 2 (g) + H 2 O(g) → CH 3 CH 2 OH(g) Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. Compare the value obtained to the value calculated from enthalpies of formation.

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Interpretation Introduction Interpretation: The enthalpy change for the given reaction has to be determined and has to be compared with the calculated value of enthalpies of formation. Concept Introduction: Bond dissociation enthalpy: Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase. Δ r H = ∑ Δ H ( b o n d s b r o k e n ) − ∑ Δ H ( b o n d s f o r m e d ) Enthalpy of formation: Δ r H = ∑ Δ f H 0 ( p r o d u c t s ) − ∑ Δ f H 0 ( reactants ) Explanation Given: H 2 C = C H 2 ( g ) + H 2 O ( g ) → C H 3 C H 2 O H ( g ) Using the bond dissociation enthalpy, we can estimate the enthalpy change for this reaction. Bond dissociation enthalpies for different bonds are given below: C-H is 413kJ/mol C=C is 610kJ/mol C-C is 346kJ/mol C-O is 358kJ/mol O-H is 463 kJ/mol . Examining the reaction shows that there are 1C=C a n d 2 O -H broken in reactant side and the bond formed in product sides are 1C-C , 1 C-H , 1 O-H and 1 C-O 1 mol ( 610 kJ/mol ) + 2 mol ( 463 kJ/mol ) → 1 mol ( 346 kJ/mol ) + 1 mol ( 413 kJ/mol ) + 1 mol ( 463 kJ/mol ) + 1 mol ( 358 kJ/mol ) 1536 kJ → 1580 kJ Δ r H = ∑ Δ H ( b o n d s b r o k e n )

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Chemistry & Chemical Reactivity

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John C. Kotz + 3 others

Publisher: Cengage Learning

ISBN: 9781133949640

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Interpretation Introduction

Interpretation: The enthalpy change for the given reaction has to be determined and has to be compared with the calculated value of enthalpies of formation.

Concept Introduction:

Bond dissociation enthalpy:

Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase.

ΔrH=∑ΔH(bonds broken)−∑ΔH(bonds formed)

Enthalpy of formation:

ΔrH=∑ΔfH0(products)−∑ΔfH0(reactants)

Explanation of Solution

Given:

H2C=CH2 (g) + H2O(g) → CH3CH2OH (g)

Using the bond dissociation enthalpy, we can estimate the enthalpy change for this reaction.

Bond dissociation enthalpies for different bonds are given below:

C-H is 413kJ/mol

C=C is 610kJ/mol

C-C is 346kJ/mol

C-O is 358kJ/mol

O-H is 463kJ/mol.

Examining the reaction shows that there are 1C=C and 2 O-H broken in reactant side and the bond formed in product sides are 1C-C , 1 C-H , 1 O-H and 1 C-O

1mol(610 kJ/mol)+2mol(463 kJ/mol)→1mol(346 kJ/mol)+1mol(413 kJ/mol) +1mol(463 kJ/mol) +1mol(358 kJ/mol)1536 kJ→1580kJ

ΔrH=∑ΔH(bonds broken)

Ethanol can be made by the reaction of ethylene and water: H 2 C=CH 2 (g) + H 2 O(g) → CH 3 CH 2 OH(g) Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. Compare the value obtained to the value calculated from enthalpies of formation.

Chemistry & Chemical Reactivity

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Chemistry & Chemical Reactivity

Ethanol can be made by the reaction of ethylene and water:

H₂C=CH₂(g) + H₂O(g) → CH₃CH₂OH(g)

Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. Compare the value obtained to the value calculated from enthalpies of formation.

Explanation of Solution

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Ethanol can be made by the reaction of ethylene and water: H 2 C=CH 2 (g) + H 2 O(g) → CH 3 CH 2 OH(g) Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. Compare the value obtained to the value calculated from enthalpies of formation.

Chemistry & Chemical Reactivity

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Chemistry & Chemical Reactivity