In the gas phase, methyl isocyanate (CH₃NC)isomerizes to acetonitrile (CH₃CN), H₃C-N$\equiv$C (g) 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. A)1.68 × 10^-10 B)5.96 × 10⁹ C)2.16 × 10¹⁰ D)4.63 × 10^-11 E)8.64 × 10¹²

Question

Quizplus · Accepted Answer

The equilibrium constant (K) can be calculated using the equation:

K = e^(-ΔG°/RT)

where R is the gas constant (8.314 J/mol∙K), T is the temperature in Kelvin, and ΔG° is the standard free energy change.

At 25°C (298 K), the value of ΔG° is -73.8 kJ/mol, so:

K = e^(-(-73.8*1000)/(8.314*298)) = 5.96 x 10^19

At 100°C (373 K), the equation becomes:

K = e^(-(-73.8*1000)/(8.314*373)) = 1.68 x 10^-10

Therefore, the best choice is B.

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

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