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Q. No.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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| 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 reaction:
\(A(g) \xrightarrow{k=0.1 M \min ^{-1}} 2 B(\mathrm{~g}) \)
If the initial concentration of A is 0.5 M, which of the following graphs correctly represents the concentration of B over time?
\(A(g) \xrightarrow{k=0.1 M \min ^{-1}} 2 B(\mathrm{~g}) \)
If the initial concentration of A is 0.5 M, which of the following graphs correctly represents the concentration of B over time?
| 1. |  |
2. |  |
| 3. |  |
4. |  |
Subtopic: Definition, Rate Constant, Rate Law |
Level 3: 35%-60%
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The rate of reaction will be fast if:
1. \(\Delta G^\circ\) is a large negative number
2. \(\Delta S^\circ\) is a large negative number
3. \(\Delta H^\circ\) is a large negative number
4. None of the above can be used to estimate reaction rates.
1. \(\Delta G^\circ\) is a large negative number
2. \(\Delta S^\circ\) is a large negative number
3. \(\Delta H^\circ\) is a large negative number
4. None of the above can be used to estimate reaction rates.
Subtopic: Definition, Rate Constant, Rate Law |
54%
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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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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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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The forward rate constant for an elementary reversible gaseous reaction is given as
\(\mathrm{C}_2 \mathrm{H}_6 \rightleftharpoons 2 \mathrm{CH}_3 \text { is } 1.57 \times 10^{-3} \mathrm{~s}^{-1} \text { at } 100 \mathrm{~K}\)
What is the rate constant for the backward reaction at this temperature if \(10^{-4}\) moles of \(\mathrm{CH}_3\) and \(10\) moles of \(\mathrm{C}_2 \mathrm{H}_6\) are present in a \(10\) litre vessel at equilibrium?
1. \(1.57 \times 10^9 \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1}\)
2. \(1.57 \times 10^{10} \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1}\)
3. \(1.57 \times 10^{11} \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1}\)
4. \(1.57 \times 10^7 \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1}\)
Subtopic: Definition, Rate Constant, Rate Law |
66%
Level 2: 60%+
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Q. No.
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