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Q. No.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:
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%
From NCERT
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. \( \dfrac{-\Delta[\mathrm{H}]}{\Delta t}=\dfrac{\Delta\left[\mathrm{H}_2\right]}{\Delta t}\)
\(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)
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. \( \dfrac{-\Delta[\mathrm{H}]}{\Delta t}=\dfrac{\Delta\left[\mathrm{H}_2\right]}{\Delta t}\)
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
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%
From NCERT
NEET - 2024
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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 |
72%
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NEET - 2024
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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.
\(4A\,+\,2B\) → \(C \,+\,3D\)
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 |
From NCERT
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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:
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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NEET - 2023
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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 |
78%
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NEET - 2023
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