The half-life for radioactive decay of ^{14}C is 5730 years. A wood sample contains only 80% of the ^{14}C .The age of the wood sample would be-

1. 1898 years

2. 1765 years

3. 1931 years

4. 1860 years

From NCERT

Subtopic: First Order Reaction Kinetics |

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The rate constant for the decomposition of hydrocarbons is 2.418 × 10^{–5 }s^{–1} at 546 K. If the energy of activation is 179.9 kJ/mol,
the value of the pre-exponential factor will be

$1.4.0\times {10}^{12}{\mathrm{s}}^{-1}\phantom{\rule{0ex}{0ex}}2.7.8\times {10}^{-13}{\mathrm{s}}^{-1}\phantom{\rule{0ex}{0ex}}3.3.8\times {10}^{-12}{\mathrm{s}}^{-1}\phantom{\rule{0ex}{0ex}}4.4.7\times {10}^{12}{\mathrm{s}}^{-1}$

From NCERT

Subtopic: Arrhenius Equation |

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For a reaction A → Product, with k = 2.0 × 10^{–2}s^{–1}, if the initial concentration of A is 1.0 mol L^{-1} , the concentration of A after 100 seconds would be

1. 0.23 mol L^{-1}

2. 0.18 mol L^{-1}

3. 0.11 mol L^{-1}

4. 0.13 mol L^{-1}

From NCERT

Subtopic: First Order Reaction Kinetics |

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The decomposition of sucrose follows the first-order rate law. For this decomposition, t_{1/2} is 3.00 hours.
The fraction of a sample of sucrose that remains after 8 hours would be:

1. 0.13

2. 0.42

3. 0.16

4. 0.25

Subtopic: First Order Reaction Kinetics |

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The decomposition of hydrocarbons follows the equation: k = (4.5 × 10^{11}s^{–1}) e^{-28000K/T}

The activation energy (E_{a}) for the reaction would be:

1. 232.79 kJ mol^{-1}

2. 245.86 kJ mol^{-1}

3. 126.12 kJ mol^{-1}

4. 242.51 kJ mol^{-1}

Subtopic: Arrhenius Equation |

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The rate constant for the first-order decomposition of H_{2}O_{2} is given by the equation: log k = 14.34 – 1.25 × 10^{4}$\frac{\mathrm{K}}{\mathrm{T}}$.
The value of E_{a} for the reaction would be:

1. 249.34 kJ mol^{-1}

2. 242.64 J mol^{-1}

3. -275.68 kJ mol^{-1}

4. 239.34 kJ mol^{-1}

Subtopic: Arrhenius Equation |

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The decomposition of A into the product has a value of k as 4.5 × 10^{3} s^{–1} at 10°C and energy of activation of 60 kJ mol^{–1}. The temperature at which the rate constant becomes 1.5 × 10^{4 }s^{–1 }would be -

$1.24\mathrm{K}\phantom{\rule{0ex}{0ex}}2.24\xb0\mathrm{C}\phantom{\rule{0ex}{0ex}}3.31\xb0\mathrm{C}\phantom{\rule{0ex}{0ex}}4.38\xb0\mathrm{C}$

Subtopic: Arrhenius Equation |

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The rate of a reaction quadruples when the temperature changes from 293 K to 313 K. The energy of activation of the reaction would be -

1. 65.93 kJ mol^{-1}

2. 52.85 kJ mol^{-1}

3. 55.46 kJ mol^{-1}

4. 60.93 kJ mol^{-1}

Subtopic: Arrhenius Equation |

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The decomposition of NH_{3} on a platinum surface is a zero-order reaction. The rates of production of N_{2} and H_{2} if k = 2.5 × 10^{–4} mol^{–1} L s^{–1} will be respectively:

1. 2.5 x 10^{-4} mol L^{-1} s^{-1} and 5.5 x 10^{-4} mol L^{-1} s^{-1}

2. 2.5 x 10^{-4} mol L^{-1} s^{-1} and 7.5 x 10^{-4} mol L^{-1} s^{-1}

3. 1.5 x 10^{-4} mol L^{-1} s^{-1} and 4.5 x 10^{-4} mol L^{-1} s^{-1}

4. 0.5 x 10^{-4} mol L^{-1} s^{-1} and 3.5 x 10^{-4} mol L^{-1} s^{-1}

Subtopic: Definition, Rate Constant, Rate Law |

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The rate equation of a reaction is expressed as, Rate=K $({\mathrm{P}}_{{\mathrm{CH}}_{3}{\mathrm{OCH}}_{3}}{)}^{\raisebox{1ex}{$3$}\!\left/ \!\raisebox{-1ex}{$2$}\right.}$

(Unit of rate = bar min^{-1})

The units of the rate constant will be:

$1.{\mathrm{bar}}^{1/2}\mathrm{min}\phantom{\rule{0ex}{0ex}}2.{\mathrm{bar}}^{2}{\mathrm{min}}^{-1}\phantom{\rule{0ex}{0ex}}3.{\mathrm{bar}}^{-1}{\mathrm{min}}^{-2}\phantom{\rule{0ex}{0ex}}4.{\mathrm{bar}}^{-1/2}{\mathrm{min}}^{-1}$

Subtopic: Definition, Rate Constant, Rate Law |

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