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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The decomposition of hydrocarbons follows the equation: k = (4.5 × 1011s–1) e-28000K/T

The activation energy (Ea) 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 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 mol-1

3. -275.68 kJ mol-1

4. 239.34 kJ mol-1

Subtopic:  Arrhenius Equation |
 56%
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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 -

124 K
2. 24 °C
3. 31 °C
4. 38 °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 correct statement about the rate constant of a reaction is:

1. Rate constant is nearly doubled with a rise in temperature by 10 °C 
2. Rate constant becomes half with a rise in temperature by 10 °C 
3. Rate constant remains unchanged with a rise in temperature by 10 °C 
4. None of the above
Subtopic:  Arrhenius Equation |
 87%
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A first-order reaction's 10 percent completion time at 298 K is the same as its 25 percent completion time at 308 K. The value of Ea will be:

1. 76.64 J mol-1

2. 66.64 kJ mol-1

3. 76.64 kJ mol-1

4. 70.34 kJ mol-1

Subtopic:  Arrhenius Equation |
 52%
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