12.1 Exercise 3

In the nuclear industry, chlorine trifluoride is used to prepare uranium hexafluoride, a volatile compound of uranium used in the separation of uranium isotopes. Chlorine trifluoride is prepared by the reaction $\text{Cl}_{2} \left(g\right) + \text{3F}_{2} \left(g\right) \rightarrow \text{2ClF}_{3} \left(g\right) .$ Write the equation that relates the rate expressions for this reaction in terms of the disappearance of Cl₂ and F₂ and the formation of ClF₃.