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Q. No.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%
Level 2: 60%+
NEET - 2024
Hints
Which plot of In k vs \(\frac{\text{I}}{\text{T}}\) is consistent with Arrhenius equation?
| 1. |  |
2. |  |
| 3. |  |
4. |  |
Subtopic: Arrhenius Equation |
71%
Level 2: 60%+
NEET - 2024
Hints
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
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%
Level 3: 35%-60%
NEET - 2024
Hints
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 |
90%
Level 1: 80%+
NEET - 2024
Hints
Effective collisions are known to possess:
A: Energy greater than the threshold energy.
B: Breaking of old bonds in the reactant.
C: Formation of a new bond in the product.
D: High activation energy.
E: Proper orientation.
Choose the correct answer from the options given below:
A: Energy greater than the threshold energy.
B: Breaking of old bonds in the reactant.
C: Formation of a new bond in the 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 |
73%
Level 2: 60%+
NEET - 2024
Hints
What is the rate constant for a reaction if the time taken by the first-order decomposition of \(\text{SO}_2\text{Cl}_2\) to decompose to 40% is 560 seconds?
[Given: log 2.5 = 0.3979]
[Given: 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. | None of the above |
Subtopic: First Order Reaction Kinetics |
Level 4: Below 35%
NEET - 2024
Hints
Given below are two statements:
| Assertion (A): | A reaction can have zero activation energy. |
| Reason (R): | The minimum amount of energy required by reactant molecules so that their energy becomes equal to threshold value, is called activation energy. |
| 1. | (A) is False but (R) is True. |
| 2. | Both (A) and (R) are True and (R) is the correct explanation of (A) |
| 3. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
| 4. | (A) is True but (R) is False. |
Subtopic: Arrhenius Equation |
Level 4: Below 35%
NEET - 2023
Hints
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 |
80%
Level 1: 80%+
NEET - 2023
Hints
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%
Level 1: 80%+
NEET - 2023
Hints
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 |
81%
Level 1: 80%+
NEET - 2023
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