The time taken by the first order decomposition of \(\text{SO}_2\text{Cl}_2\) to decompose to 40% is 560 seconds. The rate constant for the reaction is:
(log 2.5 = 0.3979)

1. \(2.726 \times 10^{-5} \mathrm{~min}^{-1}\)
2. \(2.276 \times 10^{-5} \mathrm{~min}^{-1}\)
3. \(2.216 \times 10^{-5} \mathrm{~min}^{-1}\)
4. \(2.126 \times 10^{-5} \mathrm{~min}^{-1}\)

Subtopic:  First Order Reaction Kinetics |
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NEET - 2024
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Effective collisions are known to possess:

A: Energy greater than threshold energy.
B: Breaking of old bond in reactant.
C: Formation of new bond in product.
D: High activation energy.
E: Proper orientation.

Choose the correct answer from the options given below:
1. A, B, C, D only 2. A, B, C, E only
3. A, C, D, E only 4. B, C, D, E only
Subtopic:  Arrhenius Equation |
 75%
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NEET - 2024
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Which of the following expression is correct for the reaction given below?\(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)
1. \(\dfrac{-\Delta[\mathrm{H}I]}{\Delta t}=\dfrac{2 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\) 2. \(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4\Delta\left[\mathrm{I}_2\right]}{\Delta t}\)
3. \(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\) 4. \( \dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{\Delta\left[\mathrm{H}_2\right]}{\Delta t}\)
Subtopic:  Definition, Rate Constant, Rate Law |
 92%
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NEET - 2024
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The rate of a reaction quadruples when temperature changes from 27°C to 57°C. Calculate the energy of activation.
Given R = 8.314 J K–1 mol–1, log 4 = 0.6021
1. 380.4 kJ/mol 2. 3.80 kJ/mol
3. 3804 kJ/mol 4. 38.04 kJ/mol
Subtopic:  Arrhenius Equation |
 57%
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NEET - 2024
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Which plot of In k vs \(\frac{\text{I}}{\text{T}}\) is consistent with Arrhenius equation?
1. 2.
3. 4.
Subtopic:  Arrhenius Equation |
 72%
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Activation energy of any chemical reaction can be calculated if one knows the value of: 
1. Probability of collision.
2. Orientation of reactant molecules during collision.
3. Rate constant at two different temperatures.
4. Rate constant at standard temperature.
Subtopic:  Arrhenius Equation |
 71%
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The correct rate law for the given balanced reaction is :
               \(4A\,+\,2B\) → \(C \,+\,3D\)

1. Rate = k[A]4[B]2
2. Rate = k[A]2[B]
3. Rate = k[C][D]3/[A]4[B]2
4. Cannot be determined from the information given.
Subtopic:  Definition, Rate Constant, Rate Law |
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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: 
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 |
 80%
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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 |
 80%
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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 |
 79%
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