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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 |
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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 |
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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 |
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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. \( \dfrac{-\Delta[\mathrm{H}]}{\Delta t}=\dfrac{\Delta\left[\mathrm{H}_2\right]}{\Delta t}\)
\(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)
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 |
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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
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 |
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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. \(2.126 \times 10^{-5} \mathrm{~min}^{-1}\)
(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 |
From NCERT
NEET - 2024
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The following data is for a reaction between reactants A and B:
The order of the reaction with respect to A and B, respectively are:
1. 1, 0
2. 0, 1
3. 1, 2
4. 2, 1
| Rate mol \(L^{-1}s^{-1}\) |
[A] | [B] |
| \(2 \times10^{-3}\) | 0.1 M | 0.1 M |
| \(4 \times10^{-3}\) | 0.2 M | 0.1 M |
| \(1.6 \times10^{-2}\) | 0.2 M | 0.2 M |
The order of the reaction with respect to A and B, respectively are:
1. 1, 0
2. 0, 1
3. 1, 2
4. 2, 1
Subtopic: Order, Molecularity and Mechanism |
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Which of the following plot represents the variation of \(ln ~k\) versus \(\frac 1{T}\) in according with Arrhenius equation?
| 1. |  |
2. |
 |
| 3. |
 |
4. |
 |
Subtopic: Arrhenius Equation |
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Rate constants of a reaction at 500 K and 700 K are 0.04 \(s^{-1}\) and 0.14 \(s^{-1}\), respectively; then, activation energy of the reaction is:
(Given : log 3.5 = 0.5441, R = 8.31 J \(K^{-1} \) \(\mathrm {mol}^{-1}\))
1. 182310 J
2. 18500 J
3. 18219 J
4. 18030 J
(Given : log 3.5 = 0.5441, R = 8.31 J \(K^{-1} \) \(\mathrm {mol}^{-1}\))
1. 182310 J
2. 18500 J
3. 18219 J
4. 18030 J
Subtopic: Arrhenius Equation |
From NCERT
NEET - 2024
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Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R):
In the light of the above statements choose the correct answer from the options given below:
| Assertion (A): | A reaction can have zero activation energy. |
| Reason (R): | The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value, is called activation energy. |
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
| 3. | (A) is True but (R) is False. |
| 4. | (A) is False but (R) is True. |
Subtopic: Arrhenius Equation |
From NCERT
NEET - 2023
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