Q. No.Which of the following plot represents the variation of \(ln ~k\) versus \(\frac 1{T}\) according to the Arrhenius equation?
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Subtopic: Arrhenius Equation |
86%
Level 1: 80%+
NEET - 2024
Hints
Rate constants of a reaction at 500 K and 700 K are 0.04 \(s^{-1}\) and 0.14 \(s^{-1}\) respectively, then the activation energy of the reaction is:
[Given: log 3.5 = 0.5441, R = \(8.31 \text J\text K^{-1} \text{mol}^{-1}\) ]
1. 18231 J
2. 18500 J
3. 18219 J
4. 18030 J
[Given: log 3.5 = 0.5441, R = \(8.31 \text J\text K^{-1} \text{mol}^{-1}\) ]
1. 18231 J
2. 18500 J
3. 18219 J
4. 18030 J
Subtopic: Arrhenius Equation |
Level 3: 35%-60%
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 |
72%
Level 2: 60%+
NEET - 2024
Hints
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 |
69%
Level 2: 60%+
NEET - 2024
Hints
Which plot of In k vs \(\frac{\text{I}}{\text{T}}\) is consistent with Arrhenius equation?
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Subtopic: Arrhenius Equation |
69%
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
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
The plot of ln k vs \({1 \over T}\) for the following reaction, \(2N_2O_5(g) \rightarrow 4NO_2 (g) + O_2(g) \) gives a straight line with the slope of the line equal to \(-1.0 \times 10^4 K \).
What is the activation energy for the reaction in J mol–1 ?
(Given: R = 8.3 J K–1 mol–1)
| 1. | \(4.0 \times 10^2 \) | 2. | \(4.0 \times 10^{-2} \) |
| 3. | \(8.3 \times 10^{-4} \) | 4. | \(8.3 \times 10^4 \) |
Subtopic: Arrhenius Equation |
79%
Level 2: 60%+
NEET - 2022
Hints
For a reaction AB, enthalpy of reaction is and enthalpy of activation is . The correct potential energy profile for the reaction is:
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Subtopic: Arrhenius Equation |
76%
Level 2: 60%+
NEET - 2021
Hints
The slope of Arrhenius Plot (ln k v/s ) of the first-order reaction is . The value of Ea of the reaction is:
[Given R = 8.314 JK–1 mol–1]
| 1. | 166 kJ mol–1 | 2. | –83 kJ mol–1 |
| 3. | 41.5 kJ mol–1 | 4. | 83.0 kJ mol–1 |
Subtopic: Arrhenius Equation |
79%
Level 2: 60%+
NEET - 2021
Hints
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