#### Question

The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:

Experiment | A/ mol L^{−1} |
B/ mol L^{−1} |
Initial rate/mol L^{−1} min^{−1} |

I | 0.1 | 0.1 | 2.0 × 10^{−2} |

II | -- | 0.2 | 4.0 × 10^{−2} |

III | 0.4 | 0.4 | -- |

IV | -- | 0.2 | 2.0 × 10^{−2} |

#### Solution

The given reaction is of the first order with respect to A and of zero order with respect to B.

Therefore, the rate of the reaction is given by,

Rate = *k *[A]^{1} [B]^{0}

⇒ Rate = *k *[A]

From experiment I, we obtain

2.0 × 10^{−2} mol L^{−1} min^{−1} = k (0.1 mol L^{−1})

⇒ *k* = 0.2 min^{−1}

From experiment II, we obtain

4.0 × 10^{−2} mol L^{−1} min^{−1} = 0.2 min^{−1} [A]

⇒ [A] = 0.2 mol L^{−1}

From experiment III, we obtain

Rate = 0.2 min^{−1} × 0.4 mol L^{−1}

= 0.08 mol L^{−1} min^{−1}

From experiment IV, we obtain

2.0 × 10^{−2} mol L^{−1} min^{−1} = 0.2 min^{−1} [A]

⇒ [A] = 0.1 mol L^{−1}

Is there an error in this question or solution?

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The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table Concept: Integrated Rate Equations - First Order Reactions.

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