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An important industrial source of ethanol is the reaction, catalyzed by H₃PO₄, of steam with ethylene derived from oil:
C₂H₄(g) + H₂O(g) ⇄ C₂H₅OH(g)
ΔH°rxn = -47.8kj Kc = 9 ×10³ at 600K(d) In NH₃ manufacture, the yield is increased by condensing the NH₃ to a liquid and removing it. Would condensing the C₂H₅OH have the same effect in ethanol production? Explain.

Respuesta :

The ideal gas law states that the relationship between partial pressure and volume is inverse. Additionally, it relates temperature and moles in a direct proportion. The partial pressures of the gases are discovered to be at equilibrium in the following process at room temperature and to be PN2 = 0.094 atm, PH2 = 0.039 atm, and PNH3 = 0.003 atm.

What is equilibrium partial pressures?

Each reactant's equilibrium partial pressure will be equal to its stated initial partial pressure minus x. For reactions that have the first general form below or the second form, the equilibrium partial pressure of product will be x or 2x.

The equilibrium partial pressures (in the bar) of CO, H2​O, CO2​, and H2​ are 4−p,4−p, and respectively.

Let p bar be the equilibrium partial pressure of hydrogen.

The expression for the equilibrium constant is

Kp​=PCO​PH2​O​PCO2​​PH2​​​=(4−p)(4−p)p×p​=0.1

p=1.264−0.316p

p=0.96 bar.

To learn more about equilibrium partial pressures from the given link:

brainly.com/question/17049019

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