Calculate the equilibrium constant for the oxychlorination of ethylene to vinyl chloride, CH₂CHCl, under standard conditions at 100^oC given the thermodynamic data below collected at 25^oC:
$\Delta$ G° = 53.6(CH₂CHCl), -95.3(HCl), 68.49(CH₂CH₂), -228.7(H₂O) kJ/mol
$\Delta$ H° = 37.2(CH₂CHCl), -92.3(HCl), 52.4(CH₂CH₂), -241.8(H₂O) kJ/mol
The equation of reaction is:
CH₂CH₂ ₍_g₎ + HCl ₍_g₎ + $\frac{1}{2}$ O₂ ₍_g₎ $\rarr$ CH₂CHCl ₍_g₎ + H₂O ₍_g₎

Question

Calculate the equilibrium constant for the oxychlorination of ethylene to vinyl chloride, CH₂CHCl, under standard conditions at 100^oC given the thermodynamic data below collected at 25^oC:

\Delta

G° = 53.6(CH₂CHCl), -95.3(HCl), 68.49(CH₂CH₂), -228.7(H₂O) kJ/mol

\Delta

H° = 37.2(CH₂CHCl), -92.3(HCl), 52.4(CH₂CH₂), -241.8(H₂O) kJ/mol
The equation of reaction is:
CH₂CH₂ ₍_g₎ + HCl ₍_g₎ +

\frac{1}{2}

O₂ ₍_g₎

\rarr

CH₂CHCl ₍_g₎ + H₂O ₍_g₎

Quizplus · Accepted Answer

The Answer of Calculate the equilibrium constant for the oxychlorination of ethylene to vinyl chloride, CH₂CHCl, under standard conditions at 100^oC given the thermodynamic data below collected at 25^oC: $\Delta$G° = 53.6(CH₂CHCl), -95.3(HCl), 68.49(CH₂CH₂), -228.7(H₂O) kJ/mol $\Delta$H° = 37.2(CH₂CHCl), -92.3(HCl), 52.4(CH₂CH₂), -241.8(H₂O) kJ/mol The equation of reaction is: CH₂CH₂ ₍_g₎ + HCl ₍_g₎ + $\frac{1}{2}$ O₂ ₍_g₎ $\rarr$ CH₂CHCl ₍_g₎ + H₂O ₍_g₎

Calculate the Equilibrium Constant for the Oxychlorination of Ethylene to Vinyl