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The decomposition of N_{2}O_{5} in CCl_{4} at 318K has been studied by monitoring the concentration of N_{2}O_{5} in the solution. Initially, the concentration of N_{2}O_{5} is 2.33 mol L^{–1} and after 184 minutes, it is reduced to 2.08 mol L^{–1}. The reaction takes place according to the equation

2 N_{2}O_{5} (g) → 4 NO_{2} (g) + O_{2} (g)

The rate of production of NO_{2} during this period is-

1. 5.72 × 10^{–3} mol L^{–1} min^{–1}

2. 2.72 × 10^{–3} mol L^{–1} min^{–1}

3. 1.72 × 10^{–5} mol L^{–1} min^{–1}

4. 6.72 × 10^{–4} mol L^{–1} min^{–1}

Subtopic: Definition, Rate Constant, Rate Law |

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The rate equation for the reaction 2A+B→C is found to be:

rate = k [A] [B]

The correct statement in relation to this reaction is that the:

1. | Unit of k must be s^{-1} |

2. | t_{1/2} is a constant |

3. | Rate of formation of C is twice the rate of disappearance of A |

4. | Value of k is independent of the initial concentrations of A and B |

Subtopic: Definition, Rate Constant, Rate Law |

54%

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For a reaction, A + B → Product; the rate law is given by, r=k[A]^{1/2}[B]^{2}. The order of the reaction is:

1. | -1.5 | 2. | 1.5 |

3. | 0.5 | 4. | 2.5 |

Subtopic: Order, Molecularity and Mechanism |

77%

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For the reaction, A + B → Products

The rate law and unit of rate constant respectively, are:

Experiment | [A] | [B] | Rate (mole litre^{-1} min^{-1}) |

1. | 0.01 | 0.01 | 2 × 10^{-4} |

2. | 0.02 | 0.01 | 4 × 10^{-4} |

3. | 0.01 | 0.02 | 8 × 10^{-4} |

1. | Rate = K [A]^{2} [B] and litre^{2} mole^{-2} min^{-1} |

2. | Rate = K [A]^{3} and litre^{2} mole^{-2} min^{-1} |

3. | Rate = K [A] [B]^{2} and litre mole^{-1} min^{-1} |

4. | Rate = K [A] [B]^{2} and litre^{2} mole^{-2} min^{-1} |

Subtopic: Order, Molecularity and Mechanism |

70%

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For the reaction, 2A → B, rates= k[A]^{2}. If the concentration of reactant is doubled, then the:

(a) | rate of reaction will be doubled. |

(b) | rate constant will remain unchanged, however rate of reaction is directly proportional to the rate constant. |

(c) | rate constant will change since the rate of reaction and rate constant are directly proportional to each other. |

(d) | rate of reaction will increase by four times. |

Identify the set of correct statements & choose the correct answer from the options given below:

1. | (a) and (c) only | 2. | (a) and (b) only |

3. | (b) and (d) only | 4. | (c) and (d) only |

Subtopic: Definition, Rate Constant, Rate Law |

68%

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H_{2} gas is absorbed on the metal surface like gold, tungsten, etc. This follows ________ order reaction:

1. Third

2. Second

3. Zero

4. First

Subtopic: Order, Molecularity and Mechanism |

68%

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Which of the following statements is not true for the rate constant, k?

1. | large value of k indicates fast reactions. |

2. | The value of k is independent of the concentration of reactants |

3. | The value of k is independent of the concentration of products |

4. | The value of the rate constant, k, as the name suggests is always constant for a particular reaction at all temperatures. |

Subtopic: Arrhenius Equation |

71%

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The rate constant for a reaction of zero-order in A is 0.0030 mol L^{-1} s^{-1}. How long will it take for the initial concentration of A to fall from 0.10 M to 0.075 M?

1. 8.3 sec

2. 0.83 sec

3. 83 sec

4. 10.3 sec

Subtopic: Definition, Rate Constant, Rate Law |

77%

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Given the reaction, \(A + B \rightarrow Products,\) , when concentration of A is fixed and concentration of B is increased 3 times then rate of reaction increases 27 times. Now, when the concentration of A and B both are doubled, then the rate of reaction increases 8 times. The rate law for the reaction will be:

1. \(Rate = K [A]^2[B] \)

2. \(Rate = K [B]^3 \)

3. \(Rate = K [A]^3[B] \)

4. \(Rate = K [A]^3[B]^2\)

1. \(Rate = K [A]^2[B] \)

2. \(Rate = K [B]^3 \)

3. \(Rate = K [A]^3[B] \)

4. \(Rate = K [A]^3[B]^2\)

Subtopic: Order, Molecularity and Mechanism |

83%

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The plot of concentration of a reactant vs. time for a chemical reaction is shown below:

The order of this reaction with respect to the reactant is:

1. 0

2. 1

3. 2

4. not possible to determine from this plot

The order of this reaction with respect to the reactant is:

1. 0

2. 1

3. 2

4. not possible to determine from this plot

Subtopic: Order, Molecularity and Mechanism |

68%

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