For the reaction $2NO_2(g)$ $\longrightarrow$ $ 2NO(g)$ $+$ $O_2(g)$ rate constants (in $\frac{L}{mol\;s}$) have been determined for the following temperatures (in $^oC$):
| k | t |
| 10 | 410 |
| 14 | 420 |
| 18 | 430 |
| 24 | 440 |
Determine the activation energy $E_a$ on a graph!
| $ln\;k$ | $\frac{1}{T}$ |
| 2.30 | $1.464\cdot 10{-3}$ |
| 2.64 | $1.443\cdot 10{-3}$ |
| 2.89 | $1.422\cdot 10{-3}$ |
| 3.18 | $1.403\cdot 10{-3}$ |
We find:
$-\frac{E_a}{R}$ $=$ $\frac{\Delta y}{\Delta y}$ $=$ $-1.4\cdot 10^4\;K$
$E_a$ $=$ $1.2\cdot 10^5\frac{J}{mol}$
