Consider the kinetic data given in the following table for the...

Consider the kinetic data given in the following table for the reaction A + B + C \to$Product.<br /> <table border="1"> <tbody> <tr> <td>Experiment No.</td> <td>\left[A\right]\left(mol{dm}^{- 3}\right)</td> <td>\left[B\right] \left(mold{m}^{- 3}\right)$ \left[C\right] \left(mold{m}^{- 3}\right)$</td> <td>Rate of reaction \left(mold{m}^{- 3}{s}^{- 1}\right)$ $1$ $0.2$ $0.1$ $0.1$ $6.0 \times {10}^{- 5}$ $2$ $0.2$ $0.2$ $0.1$ $6.0 \times {10}^{- 5}$ $3$ $0.2$ $0.1$ $0.2$ $1.2 \times {10}^{- 4}$ $4$ $0.3$ $0.1$ $0.1$ $9.0 \times {10}^{- 5}$
The rate of the reaction for \left[A\right] = 0.15mold{m}^{- 3}, \left[B\right] = 0.25mold{m}^{- 3} and \left[C\right] = 0.15mold{m}^{- 3} is found to be $Y \times {10}^{- 5}mold{m}^{- 3}{s}^{- 1} .$ The value of $Y$ is __________