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2 \mathrm{~A}(\mathrm{~g})+3 \mathrm{~B}(\mathrm{~g})+\mathrm{C}(\mathrm{g}) \rightarrow \mathrm{D}(\mathrm{g})+\mathrm{E}(\mathrm{g})
The order of the given reaction is 7 / 2 and the experimental rate law of the given reaction is  \mathrm{K[A]^2[B]^x[C]^1} Find the value of ' \mathrm{2 x} 

Option: 1

3


Option: 2

2


Option: 3

1


Option: 4

4


Answers (1)

best_answer

For a given reaction:
\mathrm{a A+b B+c C \rightarrow}  Products
If,
Rate \mathrm{\propto[A]^p[B]^q[C]^r}
Overall order of the reaction is :

\mathrm{(p+q+r) }
So, for
\mathrm{ 2 A(g)+3 B(g)+C(g) \rightarrow D(g)+E(g) }
The experimental rate law is,

\mathrm{ R=K[A]^2[B]^x[C]^1 }

Thus, the overall order of the reaction is (2+x+1)

Order of given reaction is  \mathrm{ \frac{7}{2} }

\mathrm{ \therefore 2+x+1=\frac{7}{2} \\ }

\mathrm{ \Rightarrow x=\frac{7}{2}-3 \\ }

\mathrm{ \Rightarrow x=\frac{1}{2} \\ }

\mathrm{ \Rightarrow 2 x=1 }.

Posted by

Gaurav

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