The following results have been obtained during the kinetic studies of the reaction:

2A + B → C + D

Experiment | [A]/mol L | [B]/mol L | Initial rate of formation of D/mol L |

I | 0.1 | 0.1 | 6.0 × 10 |

II | 0.3 | 0.2 | 7.2 × 10 |

III | 0.3 | 0.4 | 2.88 × 10 |

IV | 0.4 | 0.1 | 2.40 × 10 |

Determine the Rate law and the rate constant for the reaction.

By comparing Experiment I and IV if we increase the concentration of A by 4 times then Rate also increased by 4 times. That means order with respect to A is 1.

By comparing Experiment II and III if we double the concentration of B Rate increases by 4 times that means order with respect to B is 2.

Rate law of reaction will be, Rate = k [A][B]^{2}

To find K, K = rate/[A][B]^{2} i.e. K = 6.0 × 10^{-3}/[0.1][0.1]^{2}

K = 6 mol^{-2}L^{2}sec^{-1}

__Order with respect to A and B is 1 and 2 Respectively. And value of K(rate constant) is = 6 mol ^{-2}L^{2}sec^{-1}__

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