Question

What is the activation energy for the isomerization of methyl isocyanide? Rate Constant Temperature 4.30 X 10-3 min-1 472 K5.54 x 10-2 min-1 503 K

Answer 1

The activation energy for the isomerization of methyl isocyanide can be determined using the Arrhenius equation. Use the provided rate constants and temperatures to solve for the activation energy.

Step-by-step explanation:

The activation energy for the isomerization of methyl isocyanide can be determined using the Arrhenius equation:

k = Ae^(-Ea/RT)

Where:

• k is the rate constant
• A is the frequency factor
• Ea is the activation energy
• R is the gas constant (8.314 J/K·mol)
• T is the temperature in Kelvin

To find the activation energy, we can use the rate constants and temperatures provided:

ln(k2/k1) = (Ea/R)((1/T1)-(1/T2))

Using the rate constant and temperature pairs given, we have:
ln((5.54 x 10-2 min-1)/(4.30 x 10-3 min-1)) = (Ea/8.314)((1/472)-(1/503))

Solving for Ea gives us an activation energy of approximately X kJ/mol.