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 cl2 (g) 3f2 (g) ⟶ 2clf3 (g). 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.
Answers: 1
![Rate=-\frac{d[Cl_2]}{dt}=-\frac{1}{3}\frac{d[F_2]}{dt}=+\frac{1}{2}\frac{d[ClF_3]}{dt}](/tpl/images/0380/6825/d2692.png)
![\text{Rate of disappearance of A}=-\frac{1}{a}\frac{d[A]}{dt}](/tpl/images/0380/6825/2d8eb.png)
![\text{Rate of disappearance of B}=-\frac{1}{b}\frac{d[B]}{dt}](/tpl/images/0380/6825/1e77e.png)
![\text{Rate of formation of C}=+\frac{1}{c}\frac{d[C]}{dt}](/tpl/images/0380/6825/cee4b.png)
![\text{Rate of formation of D}=+\frac{1}{d}\frac{d[D]}{dt}](/tpl/images/0380/6825/7ef32.png)
![Rate=-\frac{1}{a}\frac{d[A]}{dt}=-\frac{1}{b}\frac{d[B]}{dt}=+\frac{1}{c}\frac{d[C]}{dt}=+\frac{1}{d}\frac{d[D]}{dt}](/tpl/images/0380/6825/d4b94.png)
![\text{Rate of disappearance of }Cl_2=-\frac{d[Cl_2]}{dt}](/tpl/images/0380/6825/4403e.png)
![\text{Rate of disappearance of }F_2=-\frac{1}{3}\frac{d[F_2]}{dt}](/tpl/images/0380/6825/c24a1.png)
![\text{Rate of formation of }ClF_3=+\frac{1}{2}\frac{d[ClF_3]}{dt}](/tpl/images/0380/6825/1400a.png)
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In the nuclear industry, chlorine trifluoride is used to prepare uranium hexafluoride, a volatile co...
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