The reaction C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, 𝑘, is 6.1×10^−8 s^−1. What is the value of the rate constant at 805.0 K?

Answer 1

Use the Arrhenius equation

ln k₂ - ln k₁ = E_a/R (1/T₁ - 1/T₂)

Solve for k₂ remembering to change E_a to J/mol to match units of R (8.314 J/K/mol)