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Q. No.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
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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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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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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| 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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Assertion(A): The catalyst can increase that 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
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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Which of the following statements is always true about the kinetics of a chemical reaction?
| 1. | The rate law includes all reactants in the balanced overall equation. |
| 2. | The overall order equals the sum of the reactant coefficients in the overall reaction. |
| 3. | The overall order equals the sum of the reactant coefficients in the slow step of the reaction. |
| 4. | The structure of the catalyst remains unchanged throughout the reaction progress. |
Subtopic: Definition, Rate Constant, Rate Law |
Level 4: Below 35%
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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
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%
Hints
Which of the following statements is true regarding the nature of reaction order and reaction mechanisms?
| 1. | A second-order reaction is always a multistep reaction. |
| 2. | A zero-order reaction is a multistep reaction. |
| 3. | A first-order reaction is always a single-step reaction. |
| 4. | A zero-order reaction is a single-step reaction. |
Subtopic: Order, Molecularity and Mechanism |
Level 3: 35%-60%
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