Question

$2A\left(g\right)+5B\left(g\right)+3C\left(g\right)\to D\left(g\right)+E\left(g\right)$
The order of the given reaction is $\frac{9}{2}$ and the experimental rate law of the given reaction is found out to be
$K\left[A{]}^{1.5}\right[B{]}^x[C{]}^{1.5}$.
Find the value of $x$

• A. 0
• B. +1
• C. -1.5
• D. +1.5

Answer 1

The correct option is D +1.5

Order of a reaction:
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
$2A\left(g\right)+5B\left(g\right)+3C\left(g\right)\to D\left(g\right)+E\left(g\right)$

The experimental rate law is,
$r=K\left[A{]}^{1.5}\right[B{]}^x[C{]}^{1.5}$.

Thus, the overall order of the reaction is
$(1.5+x+1.5)$

Order of given reaction is $\frac{9}{2}$
$\therefore$
$\Rightarrow 3+x=\frac{9}{2}$
$x=1.5$
Thr order of reaction with respect to B is 1.5