An atmospheric chemist investigates the rate of the thermal decomposition of ozone, 2O3(g)→3O2(g)2\text{O}_3(\text{g}) \rightarrow 3\text{O}_2(\text{g})2O3(g)→3O2(g), at different temperatures. A plot of ln(k)\ln(k)ln(k) against 1/T 1/T\,1/T is constructed, where k k\,k is the rate constant and T T\,T is the temperature in K\text{K}K.
The gradient of the resulting straight line is determined to be −11 200 K-11\,200\text{ K}−11200 K.
What is the activation energy, in kJ mol−1\text{kJ mol}^{-1}kJ mol−1, for this reaction? (Use the gas constant R=8.314 J K−1 mol−1R = 8.314\text{ J K}^{-1}\text{ mol}^{-1}R=8.314 J K−1 mol−1)
+1.35+1.35+1.35
+93.1+93.1+93.1
+1350+1350+1350
+93 100+93\,100+93100
