Question 14.5.4: Use Arrhenius plot information to determine Ea. The rate of ......
Use Arrhenius plot information to determine E\pmb{_{a}}.
The rate of the following reaction was measured at different temperatures and rate constants were determined.
N_{2}O_{5}(g) → 2 NO_{2}(g) + ½ O_{2}(g)
Use these data to determine the activation energy for the reaction.
| Temperature (K) | k (s\pmb{^{-1}}) |
| 298 | 3.46 ×1 0^{-5} |
| 328 | 1.50 × 10^{-3} |
| 358 | 3.34 × 10^{-2} |
| 378 | 0.210 |
You are asked to determine the activation energy for a reaction.
You are given data that show the rate constant for a reaction as a function of temperature.
First, create a data table of the natural log of the rate constant and the inverse of temperature. Plot this data (lnk on the y-axis and 1/T on the x-axis) using a plotting program, and determine the equation for the straight line
Next, use the slope of the line to calculate activation energy.
slope = \frac{-E_{a}}{R}
-12,249 K = \frac{-E_{a}}{8.3145 \times 10^{-3}\text{ kJ/K} \cdot \text{mol}}
E_{a} = 102 kJ/mol
