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

1. 1898 years

2. 1765 years

3. 1931 years

4. 1860 years

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 × 1012 s-1
2. 7.8 × 10-13 s-1
3. 3.8 × 10-12 s-1
4. 4.7 × 1012 s-1

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 L1, the concentration of A after 100 seconds would be :

1. 0.23 mol L1 2. 0.18 mol L1
3. 0.11 mol L1 4. 0.13 mol L1
Subtopic:  First Order Reaction Kinetics |
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The decomposition of sucrose follows the first-order rate law. For this decomposition, t1/2 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 |
 55%
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The decomposition of hydrocarbons follows the equation: k = (4.5 × 1011s–1) e28000K/T

The activation energy (Ea) for the reaction would be:
1. 232.79 kJ mol1
2. 245.86 kJ mol1
3. 126.12 kJ mol1
4. 242.51 kJ mol1

Subtopic:  Arrhenius Equation |
 74%
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The rate constant for the first-order decomposition of H2O2 is given by the equation: 
\(log \ k \ = \ 14.34 \ - \ 1.25 \ \times \ 10^{4}\frac{K}{T}\)

The value of Ea for the reaction would be:

1. 249.34 kJ mol–1

2. 242.64 J mol1

3. –275.68 kJ mol1

4. 239.34 kJ mol1

Subtopic:  Arrhenius Equation |
 57%
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The decomposition of A into the product has a value of k as 4.5 × 103 s–1 at 10°C and energy of activation of 60 kJ mol–1. The temperature at which the rate constant becomes 1.5 × 10s–1   would be -

1. \(24 \text { K} \)
2. \(24 ^\circ \text { C} \)
3. \(31 ^\circ \text { C} \)
4. \(38 ^\circ \text { C} \)

Subtopic:  Arrhenius Equation |
 63%
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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 |
 71%
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The decomposition of NH3 on a platinum surface is a zero-order reaction. The rates of production of N2 and Hwill be respectively:
(given ; k = 2.5 × 10–4 mol–1 L s–1 ) 

1. 2.5 × 10−4 mol L−1 s−1 and 5.5 × 10−4 mol L−1 s−1

2. 2.5 × 10−4 mol L−1 s−1 and 7.5 × 10−4 mol L−1 s−1

3. 1.5 × 10−4 mol L−1 s−1 and 4.5 × 10−4 mol L−1 s−1

4. 0.5 × 10−4 mol L−1 s−1 and 3.5 × 10−4 mol L−1 s−1

Subtopic:  Definition, Rate Constant, Rate Law |
 80%
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The rate equation of a reaction is expressed as, Rate = \(k(P_{CH_{3}OCH_{3}})^{\frac{3}{2}}\)

(Unit of rate = bar min–1)

The units of the rate constant will be:
1. bar1/2 min    
2. bar2 min1   
3. barmin2  
4. bar1/2 min1

Subtopic:  Definition, Rate Constant, Rate Law |
 78%
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