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The activation energy for the reaction 2HI(g) → H2 + I2(g) is 209.5 kJ mol−1 at 581K. The fraction of molecules of reactants having energy equal to or greater than activation energy is-
1. 2.67 × 10−19
2. 3.57 × 10−18
3. 4.67 × 10−17
4. 1.47 × 10−19
Subtopic: Arrhenius Equation |
Level 3: 35%-60%
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What is the pre-exponential factor for a reaction at 500 K with a rate constant of 0.02 s⁻¹ and an activation energy of 18.230 kJ?
1. 1.61
2. 1.41
3. 1.81
4. 1.21
1. 1.61
2. 1.41
3. 1.81
4. 1.21
Subtopic: Arrhenius Equation |
Level 3: 35%-60%
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Given below are two statements:
Assertion(A): The catalyst can increase the rate constant to a large extent.
Reason(R): By using a suitable catalyst, we can increase the rate of reaction.
1. Both A and R are correct and R is the correct explanation of A.
2. Both A and R are correct but R is not the correct explanation of A.
3. A is true and R is false
4. A is false and R is true
Assertion(A): The catalyst can increase the rate constant to a large extent.
Reason(R): By using a suitable catalyst, we can increase the rate of reaction.
1. Both A and R are correct and R is the correct explanation of A.
2. Both A and R are correct but R is not the correct explanation of A.
3. A is true and R is false
4. A is false and R is true
Subtopic: Catalyst |
Level 3: 35%-60%
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| Assertion(A): | For exothermic reaction equilibrium constant decreases with an increase in temperature. |
| Reason(R): | For a reaction, the rate constant decreases with decrease in temperature. |
| 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 and (R) is False |
| 4. | (A) is False and (R) is True |
Subtopic: Definition, Rate Constant, Rate Law |
54%
Level 3: 35%-60%
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Consider the given two statements:
| Assertion(A): | The active complex is an intermediate product. |
| Reason(R): | The active complex is unstable because of high 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 |
Level 4: Below 35%
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Read the following statements:
The correct statements are:
1. (i), (ii)
2. (i), (iii), (iv)
3. (ii), (iii), (iv)
4. (i), (ii), (iii), (iv)
| (i) | The thermal decomposition of HI on a gold surface follows a zero-order reaction. |
| (ii) | Instantaneous rate = \(\operatorname{limit}_{t \rightarrow 0} \frac{\Delta C}{\Delta t}\) |
| (iii) | The rate of 1st order reaction is proportional to the first power of the concentration of the reactant. |
| (iv) | Radioactive reaction follows 1st order kinetics. |
1. (i), (ii)
2. (i), (iii), (iv)
3. (ii), (iii), (iv)
4. (i), (ii), (iii), (iv)
Subtopic: Definition, Rate Constant, Rate Law | First Order Reaction Kinetics |
Level 3: 35%-60%
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For the reaction A + B → C, experiments were performed in the presence of a large amount of B to measure the initial reaction rate (Vf) as a function of the initial concentration of A ([A]0). The data from the experiments are plotted as shown below. The order of the reaction with respect to A is:
1. 1
2. 3
3. 2/3
4. 3/2
1. 1
2. 3
3. 2/3
4. 3/2
Subtopic: Definition, Rate Constant, Rate Law |
Level 3: 35%-60%
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Thermal decomposition of \(Cl_2O_7\) at 400 K in the gaseous phase to \(Cl_2\) and \(O_2\) is a first order reaction with rate constant \(6.932 \times 10^{-3} s^{-1}\). The time (in minutes) required for 90% decomposition of \(Cl_2O_7\) at 400 K is:
| 1. | 5.54 | 2. | 16.61 |
| 3. | 33.32 | 4. | 332.2 |
Subtopic: Definition, Rate Constant, Rate Law |
Level 3: 35%-60%
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Consider the reaction, 2A + B → Products.
When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:
1. L mol–1 s–1
2. no unit
3. mol L–1s–1
4. s–1
Subtopic: Order, Molecularity and Mechanism |
Level 3: 35%-60%
JEE
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Sucrose hydrolysis in an acidic solution into glucose and fructose follows the first-order rate law with a half-life of 3.33 h at 25°C. After 9 h, the fraction of sucrose remaining is f. The value of \(log(\frac{1}{f})\) is A×10-2 . The value of A is:
(Rounded off to the nearest integer) [Assume : ln 10 = 2.303, ln 2 = 0.693]
1. 78
2. 81
3. 85
4. 75
Subtopic: First Order Reaction Kinetics |
72%
Level 2: 60%+
JEE
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