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Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R):

In the light of the above statements choose the correct answer from the options given below:

Assertion (A): |
A reaction can have zero activation energy. |

Reason (R): |
The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value, is called activation energy. |

1. | Both (A) and (R) are true and (R) is the correct explanation of (A). |

2. | Both (A) and (R) are true but (R) is not the correct explanation of (A). |

3. | (A) is true but (R) is false. |

4. | (A) is false but (R) is true. |

Subtopic: Arrhenius Equation |

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NEET - 2023

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For a certain reaction, the rate = \(k[A]^2[B],\) when the initial concentration of A is tripled keeping the concentration of B constant, the initial rate would be:

1. | increase by a factor of three |

2. | decrease by a factor of nine |

3. | increase by a factor of six |

4. | increase by a factor of nine |

Subtopic: Order, Molecularity and Mechanism |

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NEET - 2023

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The correct options for the rate law that corresponds to overall first order reaction is:

1. | \( Rate =k[A]^0[B]^2 \) | 2. | \( Rate =k[A][B] \) |

3. | \(Rate=k[A]^{1 / 2}[B]^2 \) | 4. | \(Rate =k[A]^{-1 / 2}[B]^{3 / 2}\) |

Subtopic: Order, Molecularity and Mechanism |

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NEET - 2023

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For a reaction \(3A \rightarrow 2B\)

The average rate of appearance of B is given by \(\Delta [B] \over \Delta t\).

The correct relation between the average rate of appearance of B with the average rate of disappearance of A is:

The average rate of appearance of B is given by \(\Delta [B] \over \Delta t\).

The correct relation between the average rate of appearance of B with the average rate of disappearance of A is:

1. | \(-\Delta [A] \over \Delta t\) | 2. | \(-3\Delta [A] \over 2\Delta t\) |

3. | \(-2\Delta [A] \over 3\Delta t\) | 4. | \(\Delta [A] \over \Delta t\) |

Subtopic: Definition, Rate Constant, Rate Law |

78%

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NEET - 2023

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The given graph is a representation of the kinetics of a reaction.

The y and x axes for zero and first-order reactions, respectively are

The y and x axes for zero and first-order reactions, respectively are

1. | zero order (y=rate and x=concentration), first order (y=rate and x=t_{1/2}) |

2. | zero order (y=concentration and x=time), first order (y=t_{1/2} and x = concentration) |

3. | zero order (y=concentration and x= time), first order (y=rate constant and x= concentration) |

4. | zero order (y=rate and x=concentration), first order (y=t_{1/2} and x = concentration) |

Subtopic: Order, Molecularity and Mechanism |

60%

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For a first-order reaction A \(\rightarrow\) Products, initial concentration of A is 0.1 M, which becomes 0.001 M after 5 minutes. Rate constant for the reaction in min^{-1} is

1. | 0.2303 | 2. | 1.3818 |

3. | 0.9212 | 4. | 0.4606 |

Subtopic: First Order Reaction Kinetics |

69%

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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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The plot of ln k vs \({1 \over T}\) for the following reaction

\(2N_2O_5(g) \rightarrow 4NO_2 (g) + O_2(g) \) gives a straight line with the slope of the line equal to \(-1.0 \times 10^4 K \).

The activation energy for the reaction in J mol^{–1} is:

(Given R = 8.3 J K^{–}^{1} mol^{–}^{1})

1. \(4.0 \times 10^2 \)

2. \(4.0 \times 10^{-2} \)

3. \(8.3 \times 10^{-4} \)

4. \(8.3 \times 10^4 \)

Subtopic: Arrhenius Equation |

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The half-life of a first-order reaction is 2000 years. If the concentration after 8000 years is 0.02 M, then the initial concentration was:

1. | 0.16 M | 2. | 0.32 M |

3. | 0.08 M | 4. | 0.04 M |

Subtopic: First Order Reaction Kinetics |

61%

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For a chemical reaction, 4A + 3B → 6C + 9D

rate of formation of C is 6 × 10^{–2} mol L^{–1} s^{–1} and rate of disappearance of A is 4 × 10^{–2} mol L^{–1} s^{–1}. The rate of reaction and amount of B consumed in interval of 10 seconds, respectively will be:

rate of formation of C is 6 × 10

1. | 1 × 10^{–2} mol L^{–1} s^{–1} and 30 × 10^{–2} mol L^{–1} |

2. | 10 × 10^{–2} mol L^{–1} s^{–1} and 10 × 10^{–2} mol L^{–1} |

3. | 1 × 10^{–2} mol L^{–1} s^{–1} and 10 × 10^{–2} mol L^{–1} |

4. | 10 × 10^{–2} mol L^{–1} s^{–1} and 30 × 10^{–2} mol L^{–1} |

Subtopic: Definition, Rate Constant, Rate Law |

68%

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