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

Experiment No.	[A] (mol $d{m}^{-3}$ )	[B] (mol $d{m}^{-3}$ )	[C] (mol $d{m}^{-3}$ )	Rate of reaction (mol $d{m}^{-3} s^{-1}$ )
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 [A] = 0.15 mol $d{m}^{-3},$ [B] = 0.25 mol $d{m}^{-3}$ and [C] = 0.15 mol $d{m}^{-3}$ is found to be $Y\times {10}^{-5}$ mol $d{m}^{-3}{s}^{-1}.$ The value of Y is______