A commercial process for preparing ethanol, C,H50H(9) , involves the process of passing ethylene gas, C2H4(9), and steam, H,0(9) over a catalyst (to increase the reaction rate). The reaction is given below: нн H. H H, H-C-ċ-H AHxn = kJ H H. н он a) Use Bond Energies to calculate the change in enthalpy (AHxn) for this reaction: Bond Bond Energies C-C 346 kJ/mol C=C 602 kJ/mol C-H 411 kJ/mol C-O 358 kJ/mol О-Н 459 kJ/mol AHrxn = Z B.E. (bonds broken) - E B.E. (bonds formed) • The sum of the Bond Energies Broken: [ Select ) kJ • The sum of the Bond Energies Formed: ( Select) v kJ • Enthalpy of Reaction(AHXN) (from Bond Energies): [ Select] kJ b) Use the Heats of Formation (AH;°) to calculate the change in enthalpy (AHrxn) for this reaction: ΔΗ. Σ (n. ΔΗ ') productsΣ (n + Δ Η )reactants %3D rxn C;Ha(9) A Hf ° = + 52.47 kJ/mol A HE ° = - 241.8 kJ/mol CH5OH(9) A Hf ° = - 235.1 kJ/mol • Enthalpy of Reaction(AHxn ) (from Heats of Formation ): [ Select ) v kJ

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A commercial process for preparing ethanol, C2H;OH(g) , involves the process of passing ethylene gas, C,H4(g), and steam, H,0(g) over a catalyst (to increase the reaction
rate).
The reaction is given below:
H
H
H,
H*.
+ H,0
H-Ć-Ć-H
AHxn =
kJ
H
H.
H
OH
a) Use Bond Energies to calculate the change in enthalpy (AHxn) for this reaction:
Bond
Bond Energies
C-C
346 kJ/mol
C=C
602 kJ/mol
C-H
411 kJ/mol
C-O
358 kJ/mol
О-Н
459 kJ/mol
AHrxn = E B.E. (bonds broken) - E B.E. (bonds formed)
• The sum of the Bond Energies Broken:
[ Select ]
v kJ
• The sum of the Bond Energies Formed:
[ Select]
v kJ
Enthalpy of Reaction(AHrxn) (from Bond Energies):
[ Select ]
kJ
b) Use the Heats of Formation (AH°) to calculate the change in enthalpy (AHxn) for this reaction:
ΔΗη Σ (n. ΔΗ; ) products -Σ (n ο ΔΗ, Ό )reactants
CHa(9)
A Hf ° = + 52.47 kJ/mol
A Hf ° = - 241.8 kJ/mol
C2H5OH(9) A Hf ° = - 235.1 kJ/mol
Enthalpy of Reaction(AHrxn) (from Heats of Formation ):
[ Select ]
v kl
Transcribed Image Text:A commercial process for preparing ethanol, C2H;OH(g) , involves the process of passing ethylene gas, C,H4(g), and steam, H,0(g) over a catalyst (to increase the reaction rate). The reaction is given below: H H H, H*. + H,0 H-Ć-Ć-H AHxn = kJ H H. H OH a) Use Bond Energies to calculate the change in enthalpy (AHxn) for this reaction: Bond Bond Energies C-C 346 kJ/mol C=C 602 kJ/mol C-H 411 kJ/mol C-O 358 kJ/mol О-Н 459 kJ/mol AHrxn = E B.E. (bonds broken) - E B.E. (bonds formed) • The sum of the Bond Energies Broken: [ Select ] v kJ • The sum of the Bond Energies Formed: [ Select] v kJ Enthalpy of Reaction(AHrxn) (from Bond Energies): [ Select ] kJ b) Use the Heats of Formation (AH°) to calculate the change in enthalpy (AHxn) for this reaction: ΔΗη Σ (n. ΔΗ; ) products -Σ (n ο ΔΗ, Ό )reactants CHa(9) A Hf ° = + 52.47 kJ/mol A Hf ° = - 241.8 kJ/mol C2H5OH(9) A Hf ° = - 235.1 kJ/mol Enthalpy of Reaction(AHrxn) (from Heats of Formation ): [ Select ] v kl
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