Answers: 2
![\text{Rate of disappearance of A}=-\frac{1}{a}\frac{d[A]}{dt}](/tpl/images/0570/6613/2d8eb.png)
![\text{Rate of disappearance of B}=-\frac{1}{b}\frac{d[B]}{dt}](/tpl/images/0570/6613/1e77e.png)
![\text{Rate of formation of C}=+\frac{1}{c}\frac{d[C]}{dt}](/tpl/images/0570/6613/cee4b.png)
![\text{Rate of formation of D}=+\frac{1}{d}\frac{d[D]}{dt}](/tpl/images/0570/6613/7ef32.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/0570/6613/d4b94.png)
![\text{Rate of disappearance of }NH_3=-\frac{1}{4}\frac{d[NH_3]}{dt}](/tpl/images/0570/6613/523c5.png)
![\text{Rate of disappearance of }O_2=-\frac{1}{7}\frac{d[O_2]}{dt}](/tpl/images/0570/6613/a1c8e.png)
![\text{Rate of formation of }NO_2=+\frac{1}{4}\frac{d[NO_2]}{dt}](/tpl/images/0570/6613/2ef8c.png)
![\text{Rate of formation of }H_2O=+\frac{1}{6}\frac{d[H_2O]}{dt}](/tpl/images/0570/6613/4e047.png)
![Rate=-\frac{1}{4}\frac{d[NH_3]}{dt}=-\frac{1}{7}\frac{d[O_2]}{dt}=+\frac{1}{4}\frac{d[NO_2]}{dt}=+\frac{1}{6}\frac{d[H_2O]}{dt}](/tpl/images/0570/6613/c1beb.png)
![-\frac{d[O_2]}{dt}=X](/tpl/images/0570/6613/a5858.png)
![-\frac{1}{7}\frac{d[O_2]}{dt}=+\frac{1}{6}\frac{d[H_2O]}{dt}](/tpl/images/0570/6613/4bb1d.png)
![\frac{d[H_2O]}{dt}=\frac{6}{7}\frac{d[O_2]}{dt}](/tpl/images/0570/6613/0a653.png)
![\frac{d[H_2O]}{dt}=\frac{6}{7}\times X](/tpl/images/0570/6613/ac1d5.png)
![\frac{d[H_2O]}{dt}=0.857X](/tpl/images/0570/6613/0ed54.png)
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Consider the reaction: 4 NH3 + 7 O2 --> 4 NO2 + 6 H2O. At a certain instant the initial rate of d...
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