Q. No.The activation energy of a chemical reaction can be calculated by:
| 1. | Determining the rate constant at standard temperature. |
| 2. | Determining the rate constant at two temperatures. |
| 3. | Determining probability of collision. |
| 4. | Using the catalyst. |
Subtopic: Arrhenius Equation |
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Level 2: 60%+
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The correct statement based on the graph below is:
| 1. | The activation energy of the forward reaction is E1 + E2 and the product is less stable than reactant. |
| 2. | The activation energy of the forward reaction is E1 + E2 and the product is more stable than the reactant. |
| 3. | The activation energy of both forward and backward reaction is E1 + E2 and reactant is more stable than the product. |
| 4. | The activation energy of the backward reaction is E1 and the product is more stable than reactant. |
Subtopic: Arrhenius Equation |
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Level 2: 60%+
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Subtopic: Arrhenius Equation |
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Level 1: 80%+
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Consider the Arrhenius equation given below and choose the correct option:
| 1. | Rate constant increases exponentially with increasing activation energy and decreasing temperature. |
| 2. | Rate constant decreases exponentially with increasing activation energy and increasing temperature. |
| 3. | Rate constant increases exponentially with decreasing activation energy and decreasing temperature. |
| 4. | Rate constant increases exponentially with decreasing activation energy and increasing temperature. |
Subtopic: Arrhenius Equation |
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Subtopic: Arrhenius Equation |
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An incorrect statement about the collision theory of chemical reaction is:
| 1. | It considers reacting molecules or atoms to be hard spheres and ignores their structural features. |
| 2. | The number of effective collisions determines the rate of reaction. |
| 3. | The collision of atoms or molecules possessing sufficient threshold energy results in product formation. |
| 4. | Molecules should collide in the proper orientation for the collision to be effective with sufficient threshold energy and proper orientation. |
Subtopic: Arrhenius Equation |
Level 3: 35%-60%
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During decomposition of an activated complex
| (a) | Energy is always released. |
| (b) | Energy is always absorbed. |
| (c) | Energy does not change. |
| (d) | Reactants may be formed. |
The correct choice among the given is -
1. (a, b)
2. (b, c)
3. (c, d)
4. (a, d)
Subtopic: Arrhenius Equation |
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The correct statements among following about Maxwell, Boltzmann distribution of energy is -
| (a) | The fraction of molecules with the most probable kinetic energy decreases at higher temperatures |
| (b) | The fraction of molecules with the most probable kinetic energy increases at higher temperatures |
| (c) | Most probable kinetic energy increases at higher temperatures |
| (d) | Most probable kinetic energy decreases at higher temperatures |
1. (a, b)
2. (b, c)
3. (c, d)
4. (a, c)
Subtopic: Arrhenius Equation |
Level 3: 35%-60%
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The correct statements among the following regarding Maxwell, Boltzmann distribution curve of energy is -
| a. | The area under the curve must not change with an increase in temperature. |
| b. | The area under the curve increases with increase in temperature. |
| c. | Area under the curve decreases with increase in temperature. |
| d. | With an increase in temperature curve broadens and shifts to the right-hand side. |
1. (a, b)
2. (b, c)
3. (c, d)
4. (a, d)
Subtopic: Arrhenius Equation |
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Level 2: 60%+
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The correct statements among the following regarding the Arrhenius equation is/are -
| (a) | Rate of a reaction increases with an increase in temperature |
| (b) | Rate of a reaction increases with a decrease in activation energy |
| (c) | Rate constant decreases exponentially with an increase in temperature |
| (d) | Rate of reaction decreases with a decrease in activation energy |
1. (a, b)
2. (b, c)
3. (c, d)
4. (a, d)
Subtopic: Arrhenius Equation |
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Level 2: 60%+
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