In the gas phase, methyl isocyanate (CH₃NC) isomerizes to acetonitrile (CH₃CN) , H₃C-N $\equiv$ C (g) $\rarr$ H₃C-C $\equiv$ N (g)
With $\Delta$ H° = -89.5 kJ/mol and $\Delta$ G° = -73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.

Question

In the gas phase, methyl isocyanate (CH₃NC) isomerizes to acetonitrile (CH₃CN) , H₃C-N

\equiv

C (g)

\rarr

H₃C-C

\equiv

N (g)
With

\Delta

H° = -89.5 kJ/mol and

\Delta

G° = -73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.

Quizplus · Accepted Answer

The equilibrium constant can be calculated using the van't Hoff equation and the given $\Delta$G° at 25°C. The change in temperature affects the equilibrium constant, and the calculation shows that the equilibrium constant at 100°C is approximately 5.96 * 10^9.

In the Gas Phase, Methyl Isocyanate (CH3NC)isomerizes to Acetonitrile (CH3CN) ≡\equiv≡

In the Gas Phase, Methyl Isocyanate (CH₃NC)isomerizes to Acetonitrile (CH₃CN) $\equiv$