Question

$2A\left(g\right)+3B\left(g\right)+C\left(g\right)\to D\left(g\right)+E\left(g\right)$
The order of the given reaction is $\frac{7}{2}$ and the experimental rate law of the given reaction is $k\left[A{]}^2\right[B{]}^x[C{]}^1$. Find the value of ${}^{\prime }{x}^{\prime }$.

• A. $1.5$
• B. $1$
• C. $0.5$
• D. $2$

Answer 1

The correct option is C $0.5$

For a given reaction:
$aA+bB+cC\to \text{Products}$
If,
$\text{Rate}\propto \left[A{]}^p\right[B{]}^q[C{]}^r$
Overall order of the reaction is :
$(p+q+r)$
So, for
$2A\left(g\right)+3B\left(g\right)+C\left(g\right)\to D\left(g\right)+E\left(g\right)$
The experimental rate law is,
$R=K\left[A{]}^2\right[B{]}^x[C{]}^1$
Thus, the overall order of the reaction is
$(2+x+1)$
Order of given reaction is $\frac{7}{2}$
$\therefore 2+x+1=\frac{7}{2}$
$\Rightarrow x=\frac{7}{2}-3$
$\Rightarrow x=\frac{1}{2}$
Thr order of reaction with respect to B is $\frac{1}{2}$