Consider the kinetic data given in the following table for the reaction $\mathrm{A}+\mathrm{B}+\mathrm{C}\to$ Product.
 

Experiment No.	$\left[\mathrm{A}\right]$ $\left(\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }{\mathrm{d}\mathrm{m}}^{-3}\right)$	$\left[\mathrm{B}\right]$ $\left(\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }\mathrm{d}{\mathrm{m}}^{-3}\right)$	$\left[\mathrm{C}\right]$ $\left(\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }\mathrm{d}{\mathrm{m}}^{-3}\right)$	Rate of reaction $\left(\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }\mathrm{d}{\mathrm{m}}^{-3}{\mathrm{s}}^{-1}\right)$
$1$	$0.2$	$0.1$	$0.1$	$6.0\times {10}^{-5}$
$2$	$0.2$	$0.2$	$0.1$	$6.0\times {10}^{-5}$
$3$	$0.2$	$0.1$	$0.2$	$1.2\times {10}^{-4}$
$4$	$0.3$	$0.1$	$0.1$	$9.0\times {10}^{-5}$

The rate of the reaction for $\left[\mathrm{A}\right]=0.15\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }\mathrm{d}{\mathrm{m}}^{-3},\mathrm{ }\left[\mathrm{B}\right]=0.25\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }\mathrm{d}{\mathrm{m}}^{-3}$ and $\left[\mathrm{C}\right]=0.15\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }\mathrm{d}{\mathrm{m}}^{-3}$ is found to be $\mathrm{Y}\times {10}^{-5}\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }\mathrm{d}{\mathrm{m}}^{-3}{\mathrm{s}}^{-1}.$ The value of $\mathrm{Y}$ is __________

Hence, the correct answer is 6.75.