A hydrogenation reaction is carried out at 500 K. If the same reaction is carried out in presence of a catalyst at the same rate with same frequency factor, the temperature required is 400 K the activation energy of the reaction, if the catalyst lowers the activation energy barrier by 16 kJ/mol is:

1. 100 kJ/mol

2. 80 kJ/mol

3. 60 kJ/mol

4. None of th above

Subtopic: Arrhenius Equation |

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Q194:

$Consider the reaction .$

$The rate constant for two parallel reactions were found to be 10^{- 2} {dm}^{3} {mol}^{- 1} s^{- 1} and 4 x 10^{- 2} {dm}^{3} {mol}^{- 1} s^{- 1} . If the corresponding energies of activation of the parallel reaction are 100 and 120 K J / mol respecctively, the net energy of activation (E_{a}) of A is$

1. 100 kJ/mol

2. 120 kJ/mol

3. 116 kJ/mol

4. 220 kJ/mol

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Q195:

$A reaction takes place in various steps . The rate constant for first, second, third, and fifth step are k_{1}, k_{2}, k_{3} and k_{5} respectively . The overall rate constant is given by k = \frac{k_{2}}{k_{3}} {(\frac{k_{1}}{k 5})}^{1 / 2} If activation energy are 40, 60, 50, and 10 kJ / mol respectively, the overall energy of activation (kJ / mol) is :$

1. 10

2. 20

3. 25

4. None of the above

Subtopic: Arrhenius Equation |

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Q82:

$For reaction A \overset{}{\to} B, the rate constant k_{1} = A_{1} e^{- E_{a_{1}} / (RT)} and for the reaction X \to y, the rate constant k_{2} = A_{2} e^{- E_{a_{2}} / (RT)} . If A_{1} = 10^{8} A_{2} = 10^{10} a n d E_{a_{1}} = 600 cal / mol, E_{a_{2}} = 1800 cal / mol, then the temperature at which k_{1} = k_{2} is (given : R = 2 cal / K - mol)$

1. $1600 K$

2. $1200 x 4.606 K$

3. $\frac{1200}{4.606} K$

4. $\frac{600}{4.606} K$

Subtopic: Arrhenius Equation |

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Q197:

$For first - order parallel reaction k_{1} and k_{2} are 4 and 2 \min^{- 1} respectively at 300 K . If the activation energies for the formation of B and C are respectively 30, 000 and 38, 314 J / mol respectively . The temperature at which B and C will be obtained in the equimolar ratio is :$

1. 757.48 K

2. 378.74 K

3. 600.91 K

4. None of the above

Subtopic: Arrhenius Equation |

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Q198:

The activation energies of two reactions are $E_{a_{1}}$ and $E_{a_{2}}$ with $E_{a_{1}}$ > $E_{a_{2}}$ .
f the temperature of the reacting system is increased from T₁ to T₂ .
The correct relation is:

1. $\frac{K_{1}'}{K_{1}} = \frac{K_{2}'}{K_{2}}$

2. $\frac{K_{1}'}{K_{1}} > \frac{K_{2}'}{K_{2}}$

3. $\frac{K_{1}'}{K_{1}} < \frac{K_{2}'}{K_{2}}$

4. $\frac{K_{1}'}{K_{1}} < 2 \frac{K_{2}'}{K_{2}}$

Subtopic: Arrhenius Equation |

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Q199:

The units of rate constant and rate of reaction are same for :
1. First order reaction
2. Second order reaction
3. Third order reaction
4. Zero order reaction

Subtopic: Order, Molecularity and Mechanism |

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Q84:

The plot of log k vs $\frac{1}{T}$ helps to calculate :

1. Energy of activation.
2. Rate constant of reaction.
3. Order of the reaction.
4. Energy of activation as well as the frequency factor.

Subtopic: Arrhenius Equation |

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Q201:

Rate constant K = 1.2×10³ mol^–1 L s^–1 and E_a = 2.0×10² kJ mol^–1. When T $\to \infty$ , A is equal
to
1. 2.0 × 10² kJ mol^–1
2. 1.2 × 10³ mol^–1L s^–1
3. 1.2 × 10³ mol L^–1 s^–1
4. 2.4 × 10³ kJ mol^–1L s^–1

Subtopic: Arrhenius Equation |

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Q202:

The rate constant for a reaction 2×10^–2s^–1 at 300 K and 8×10^–2s^–1 at 340 K. The energy of activation of the reaction is:

1. 14.69 kJ mol^–1

2. 29.39 kJ mol^–1

3. 44.34 kJ mol^–1

4. 22.05 kJ mol^–1

Subtopic: Arrhenius Equation |

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