Chapter 4 : Chemical Kinetics

Rate=k[CH3OCH3]3/2

The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether.

i.e., Rate=k[PCH3OCH3]3/2

If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?

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t/s | 0 | 30 | 60 | 90 |

[Ester]/M. | 0.55 | 0.31 | 0.17 | 0.085 |

(ii) Calculate the pseudo first order rate constant for the hydrolysis of ester.

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t/s | 0 | 400 | 800 | 1200 | 1600 | 2000 | 2400 | 2800 | 3200 |

102×[N2O5]/molL−1 | 1.63 | 1.36 | 1.14 | 0.93 | 0.78 | 0.64 | 0.53 | 0.43 | 0.35 |

(i) Plot [N2O5] against t.

(ii) Find the half-life period for the reaction.

(iii) Draw a graph between log[N2O5] and t.

(iv) What is the rate law?

(v) Calculate the rate constant.

(vi) Calculate the half-life period from k and compare it with (ii)

(ii) Find the half-life period for the reaction.

(iii) Draw a graph between log[N2O5] and t.

(iv) What is the rate law?

(v) Calculate the rate constant.

(vi) Calculate the half-life period from k and compare it with (ii)

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A/molL−1 | 0.20 | 0.20 | 0.40 |

B/molL−1 | 0.30 | 0.10 | 0.05 |

r0/molL−1s−1 | 5.07×10−5 | 5.07×10−5 | 1.43×10−4 |

What is the order of the reaction with respect to A and B?

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t(sec) | P(mm of Hg) |

0 | 35.0 |

360 | 54.0 |

720 | 63.0 |

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(a) 200s−1; (b) 2 min−1; (c) 4year−1.

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Experiment | [A]/molL−1 | B]/molL−1 | Initial rate/ molL−1min−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 |

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(i) 2NO(g)→N2O(g); Rate=k[NO]2

(ii) H2O2(aq)+3I−(aq)+2H+→2H2O(I)+3I; Rate=k[H2O2][I−]

(iii) CH3CHO(g)→CH4(g)+CO(g); Rate=k[CH3CHO]3/2

(iv) C2H5Cl(g)→C2H4(g)+HCl(g); Rate=k[C2H5Cl]

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(i) Write differential rate equation.

(ii) How is the rate affected when the concentration of B is tripled?

(iii) How is the rate affected when the concentration of both A and B is doubled?

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2A+B→C+D

Experiment | [A]/molL−1 | [B]/molL−1 | Initial rate of formation of D/molL−1min−1 |

I | 0.1 | 0.1 | 6.0×10−3 |

II | 0.3 | 0.2 | 7.2×10−2 |

III | 0.3 | 0.4 | 2.88×10−1 |

IV | 0.4 | 0.1 | 2.40×10−2 |

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

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2A+B→A2B, the rate =k[A][B]2 with k=2.0×10−6mol−2L2s−1.

Calculate the initial rate of the reaction when [A]=0.1molL−1, [B]=0.2 molL−1. Calculate the rate of reaction after [A] is reduced to 0.06 molL−1.

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