1. Tardigrade
  2. Question
  3. Chemistry
  4. For the reaction of H2 with I2, the rate constant is 2.5 × 10-4 dm3 mol-1 s-1 at 327°C and 1.0 dm3 mol-1 s-1 at 527° C. The activation energy for the reaction, in kJ mol-1 is: (R=8.314 J K-1 mol-1)

Question Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

Q. For the reaction of $H_2$ with $I_2$, the rate constant is $2.5 \times 10^{-4} dm^3 \; mol^{-1} s^{-1} $ at $327^{\circ}C$ and $1.0 \; dm^3 \; mol^{-1} \; s^{-1}$ at $527^{\circ} C$. The activation energy for the reaction, in $kJ \; mol^{-1}$ is:
$(R=8.314\,J \; K^{-1} mol^{-1})$

JEE MainJEE Main 2019Chemical Kinetics

Solution:

$H_2(g) + I_2(g) \to 2HI(g)$
Apply Arrhenius equation
$\log \frac{K_{2}}{K_{1}} \frac{E_{a}}{2.303 R} \left( \frac{1}{600} - \frac{1}{800}\right) $
$ \log \frac{1}{2.5 \times10^{-4}} = \frac{E_{a}}{2.303 \times8.31} \left( \frac{200}{600 \times800}\right) $
$ \therefore E_{a} \approx166 $ kJ/mol