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Sahay Sir > Question Answers > JEE Adv and Mains Chemistry 41 Years Solved Video Solutions 1979 - 2019 > Chemistry > Chapter 17 - Chemical Kinetics > For the reaction of H2 with I2, the rate constant is 2.5 × 10^–4 dm^3 mol^–1 s^–1 at 327°C and 1.0 dm^3 mol^–1 s^-1 at 527°C. The activation energy for the reaction, in kJ mole^–1 is : (R = 8.314 JK^–1 mol^–1 )

For the reaction of H2 with I2, the rate constant is 2.5 × 10^–4 dm^3 mol^–1 s^–1 at 327°C and 1.0 dm^3 mol^–1 s^-1 at 527°C. The activation energy for the reaction, in kJ mole^–1 is : (R = 8.314 JK^–1 mol^–1 )

For the reaction of H2 with I2 in kJ mole^–1 is : (R = 8.314 JK^–1 mol^–1 ) the rate constant is 2.5 × 10^–4 dm^3 mol^–1 s^–1 at 327°C and 1.0 dm^3 mol^–1 s^-1 at 527°C. The activation energy for the reaction