**(a) To calculate the order of the reaction with respect to each reactant, we will use the experimental data given. **

[A](M) | Initial Rate (M/s) |

0.15 | 0.020 |

0.30 | 0.158 |

0.60 | 1.266 |

$\overline{)\frac{\mathbf{rate}\mathbf{}\mathbf{2}}{\mathbf{rate}\mathbf{}\mathbf{1}}\mathbf{=}\frac{{\left[A\right]}^{\mathbf{x}}}{{\left[A\right]}^{\mathbf{x}}}}$

*x = order*

*(Larger concentration should be on the numerator)*

**Solve for x:**

Consider the following data showing the initial rate of a reaction (A products) at several different concentrations of A.

[A](M) | Initial Rate (M/s) |

0.15 | 0.020 |

0.30 | 0.158 |

0.60 | 1.266 |

What is the order of the reaction?

Express your answer as an integer

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