The activation energy of a reaction is zero. Its rate constant at 280 K is 1.6 × 10 - 6 s - 1 , the rate constant at 300 K is

Step-by-step solution

Key Idea Arrhenius equations is given as: l o g k 2 k 1 = E a 2.303 R 1 T 1 - 1 T 2 Given, Activation energy of a reaction, E A = 0 Rate constant, k 1 = 1.6 × 10 - 6 s - 1 Temperature, T 1 = 280 K , T 2 = 300 K According to Arrhenius equation l o g k 2 1.6 × 10 - 6 = 0 2.303 R 1 280 - 1 300 l o g k 2 1.6 × 10 - 6 = 0 k 2 1.6 × 10 - 6 = antilog 0 k 2 1.6 × 10 - 6 = 1 ∴ k 2 = 1.6 × 10 - 6 s - 1