In some parts of the world, butadiene was produced from ethanol, C2H6O by the unbalanced reaction: C2H6O(g) → C4H6(g) +

[answerhappygod]

In some parts of the world, butadiene was produced from ethanol,
C2H6O by the unbalanced reaction:
C2H6O(g) → C4H6(g) + H2O(g) + H2(g)
Balance the above reaction.
I’d like you to determine whether this reaction is exo- or
endothermic, but you need more information first. The following
questions will walk you through this process.
Given the reaction and thermochemical data
below, use Hess’ Law to calculate ∆H_rxn^° for the gas-phase
combustion of butadiene.
C4H6(g) + 11/2 O2(g) → 4 CO2(g) + 3 H2O(l)
∆H_rxn^° = ? kJ
2 H2(g) + O2(g) → 2 H2O(g)

∆H_f^° = −484 kJ
C4H8(g) + 6 O2(g) → 4 CO2(g) + 4 H2O(g)
∆H_rxn^° = −2527 kJ
C4H8(g) → C4H6(g) + H2(g)

∆H_rxn^° = +132 kJ
H2O(l) → H2O(g)


∆H_vap^° = +41 kJ
Now that you know the enthalpy of combustion of
butadiene, use that value and the standard enthalpies of formation
for the other species in the reaction (see Table 6.4) to determine
the enthalpy of formation of butadiene.
Use the enthalpy of formation of butadiene to
find the enthalpy of reaction for the production of butadiene from
ethanol.
Is this reaction exo- or endothermic?
Using various techniques, it is possible to isolate butadiene from
the resulting homogenous mixture. Typically, this reaction was
performed at about 400 ℃ with a variety of metal oxide catalysts
(we’ll cover catalysts in the Spring semester). Let’s assume you’re
able to isolate 6.327 kg of butadiene at 400.0 ℃ at a pressure of
10.000 atm in a 646 L reaction vessel. This vessel is equipped with
a near-frictionless piston to accommodate volume changes; its
surroundings are also held at a pressure of 10.000 atm.
The temperature decreases to 200.0 ℃ without
changing pressure, and the butadiene sample remains in the gas
phase. What is the new volume in L?
If butadiene has a specific heat of 12.9 J
℃-1 g-1, what was the heat flow associated with the above change in
kJ?
Calculate the work for this process in
kJ.
Was work performed on or by the system?
Determine ΔH for this isobaric
(constant-pressure) cooling process in kJ mol-1.
Calculate ΔU in kJ mol-1 for this process.
If the butadiene sample was first allowed to
cool to 200.0 ℃ at constant volume, then allowed to compress to the
value of V2 calculated in #6 at constant temperature, determine the
values of ΔH and ΔU in kJ mol-1.