Saved Bookmarks
| 1. |
The activation energy of a reaction is 155326 J/ mol. The rate constant of the reaction at and 300K as a function of rate constant at 400K, obtained by the Collision theory is ____(a) k1 = 1.5 × 10^-7k2(b) k1 = 1.2 × 10^-6 k2(c) k1 = 1.5 × 10^-6 k2(d) k1 = 1.2 × 10^-7 k2 |
|
Answer» Right choice is (a) k1 = 1.5 × 10^-7k2 The explanation: By collision theory, ln((frac{k_2}{k_1}) = -frac{E}{R} (frac{1}{T_2} – frac{1}{T_1}) + 0.5ln(frac{T_2}{T_1}) ) ln((frac{k_2}{k_1}) = -frac{155326}{8.314}(frac{1}{400} – frac{1}{300}) + 0.5ln(frac{400}{300}) ) Hence, k1 = 1.5 × 10^-7k2. |
|