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Q. No.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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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 |
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Level 2: 60%+
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Two first-order reactions have half-lives in the ratio. Calculate the ratio of
the time intervals \(t_1: t_2\)where the time \(t_1\) and \(t_2\) are the time periods
for \(\left(\frac{1}{4}\right)^{\mathrm{th}}\) and \(\left(\frac{3}{4}\right)^{\mathrm{th}}\) completion of the reaction, respectively.
1. \(1: 0.301\)
2. \(0.125: 0.602\)
3. \(1: 602\)
4. None of the above
the time intervals \(t_1: t_2\)where the time \(t_1\) and \(t_2\) are the time periods
for \(\left(\frac{1}{4}\right)^{\mathrm{th}}\) and \(\left(\frac{3}{4}\right)^{\mathrm{th}}\) completion of the reaction, respectively.
1. \(1: 0.301\)
2. \(0.125: 0.602\)
3. \(1: 602\)
4. None of the above
Subtopic: First Order Reaction Kinetics |
Level 3: 35%-60%
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The Arrhenius equations for two reactions are:
A → B: k₁ = 10⁸ exp(−600/RT)
X → Y: k₂ = 10¹⁰ exp(−1800/RT)
The temperature (in Kelvin) at which k₁ = k₂ is:
(Given R = 2 cal mol⁻¹ K⁻¹)
| 1. | \(1200 \mathrm{~K}\) | 2. | \(1200 \times 4.606 \mathrm{~K}\) |
| 3. | \(\dfrac{1200}{4.606} \mathrm{~K}\) | 4. | \(\dfrac{600}{4.606} \mathrm{~K}\) |
Subtopic: Arrhenius Equation |
58%
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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A catalyst will not:
| 1. | Increase the forward reaction rate. |
| 2. | Shift the equilibrium to favor the products. |
| 3. | Alter the reaction pathway. |
| 4. | Increase the speed at which equilibrium will be achieved. |
Subtopic: Catalyst |
54%
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 |
52%
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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