Consider the reaction CO(g)+ 2H₂(g) $\rarr$ CH₃OH(l)at 25°C.
$\Delta$ G°_f (CO)= -137.3 kJ/mol
$\Delta$ G°_f (CH₃OH)= -166.3 kJ/mol
$\Delta$ H°_f (CO)= -110.5 kJ/mol
$\Delta$ H°_f (CH₃OH)= -238.7 kJ/mol
S°(CO)= 197.9 J/K·mol
S°(CH₃OH)= 126.8 J/K·mol
Calculate value of the equilibrium constant (K_p)for this reaction at 25°C.

Question

Consider the reaction CO(g)+ 2H₂(g)

\rarr

CH₃OH(l)at 25°C.

\Delta

G°_f (CO)= -137.3 kJ/mol

\Delta

G°_f (CH₃OH)= -166.3 kJ/mol

\Delta

H°_f (CO)= -110.5 kJ/mol

\Delta

H°_f (CH₃OH)= -238.7 kJ/mol
S°(CO)= 197.9 J/K·mol
S°(CH₃OH)= 126.8 J/K·mol
Calculate value of the equilibrium constant (K_p)for this reaction at 25°C.

Quizplus · Accepted Answer

The Answer of Consider the reaction CO(g)+ 2H₂(g) $\rarr$ CH₃OH(l)at 25°C. $\Delta$G°_f (CO)= -137.3 kJ/mol $\Delta$G°_f (CH₃OH)= -166.3 kJ/mol $\Delta$H°_f (CO)= -110.5 kJ/mol $\Delta$H°_f (CH₃OH)= -238.7 kJ/mol S°(CO)= 197.9 J/K·mol S°(CH₃OH)= 126.8 J/K·mol Calculate value of the equilibrium constant (K_p)for this reaction at 25°C.

Consider the Reaction CO(g)+ 2H2(g) →\rarr→ CH3OH(l)at 25°C Δ\DeltaΔ G°f (CO)= -137 Δ\DeltaΔ

Consider the Reaction CO(g)+ 2H₂(g) $\rarr$ CH₃OH(l)at 25°C $\Delta$ G°_f (CO)= -137 $\Delta$