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Q. No.If the rate constant of a reaction is \(0.03 s^{-1}\) how much time does it take for \(7.2\text { mol L}^{-1}\) concentration of the reactant to get reduced to \(0.9~\text {mol L} ^{-1}\)
(Given: log 2=0.301)
1. 210 s
2. 21.0 s
3. 69.3 s
4. 23.1 s
(Given: log 2=0.301)
1. 210 s
2. 21.0 s
3. 69.3 s
4. 23.1 s
Subtopic: First Order Reaction Kinetics |
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Level 2: 60%+
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\(C(s) + 2 H_2(g) \rightarrow CH_4(g); \Delta H = -74.8kJ mol^{-1}\)
Which of the following diagrams gives an accurate representation of the above reaction?
[ R→reactants; P→products]
Which of the following diagrams gives an accurate representation of the above reaction?
[ R→reactants; P→products]
| 1. |  |
2. |  |
| 3. |  |
4. |  |
Subtopic: Arrhenius Equation |
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Level 2: 60%+
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If the half-life \((t_{1/2})\) for a first order reaction is \(1~\text{minute}\), then the time required for \(99.9 \%\) completion of the reaction is closest to :
1. \(5~\text{minutes}\)
2. \(10~\text{minutes}\)
3. \(2~\text{minutes}\)
4. \(4~\text{minutes}\)
1. \(5~\text{minutes}\)
2. \(10~\text{minutes}\)
3. \(2~\text{minutes}\)
4. \(4~\text{minutes}\)
Subtopic: First Order Reaction Kinetics |
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Level 2: 60%+
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Activation energy of any chemical reaction can be calculated if one knows the value of:
| 1. | Probability of collision. |
| 2. | Orientation of reactant molecules during collision. |
| 3. | Rate constant at two different temperatures. |
| 4. | Rate constant at standard temperature. |
Subtopic: Arrhenius Equation |
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Level 2: 60%+
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Which plot of In k vs \(\frac{\text{I}}{\text{T}}\) is consistent with Arrhenius equation?
| 1. |  |
2. |  |
| 3. |  |
4. |  |
Subtopic: Arrhenius Equation |
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The rate of a reaction quadruples when temperature changes from 27°C to 57°C. Calculate the energy of activation.
Given R = 8.314 J K–1 mol–1, log 4 = 0.6021
Given R = 8.314 J K–1 mol–1, log 4 = 0.6021
| 1. | 380.4 kJ/mol | 2. | 3.80 kJ/mol |
| 3. | 3804 kJ/mol | 4. | 38.04 kJ/mol |
Subtopic: Arrhenius Equation |
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Which of the following expression is correct for the reaction given below?\(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)
| 1. | \(\dfrac{-\Delta[\mathrm{H}I]}{\Delta t}=\dfrac{2 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\) | 2. | \(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4\Delta\left[\mathrm{I}_2\right]}{\Delta t}\) |
| 3. | \(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\) | 4. | \( \dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{\Delta\left[\mathrm{H}_2\right]}{\Delta t}\) |
Subtopic: Definition, Rate Constant, Rate Law |
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Effective collisions are known to possess:
A: Energy greater than threshold energy.
B: Breaking of old bond in reactant.
C: Formation of new bond in product.
D: High activation energy.
E: Proper orientation.
Choose the correct answer from the options given below:
A: Energy greater than threshold energy.
B: Breaking of old bond in reactant.
C: Formation of new bond in product.
D: High activation energy.
E: Proper orientation.
Choose the correct answer from the options given below:
| 1. | A, B, C, D only | 2. | A, B, C, E only |
| 3. | A, C, D, E only | 4. | B, C, D, E only |
Subtopic: Arrhenius Equation |
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The time taken by the first order decomposition of \(\text{SO}_2\text{Cl}_2\) to decompose to 40% is 560 seconds. The rate constant for the reaction is:
(log 2.5 = 0.3979)
1. \(2.726 \times 10^{-5} \mathrm{~min}^{-1}\)
2. \(2.276 \times 10^{-5} \mathrm{~min}^{-1}\)
3. \(2.216 \times 10^{-5} \mathrm{~min}^{-1}\)
4. \(2.126 \times 10^{-5} \mathrm{~min}^{-1}\)
(log 2.5 = 0.3979)
1. \(2.726 \times 10^{-5} \mathrm{~min}^{-1}\)
2. \(2.276 \times 10^{-5} \mathrm{~min}^{-1}\)
3. \(2.216 \times 10^{-5} \mathrm{~min}^{-1}\)
4. \(2.126 \times 10^{-5} \mathrm{~min}^{-1}\)
Subtopic: First Order Reaction Kinetics |
Level 3: 35%-60%
NEET - 2024
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The following data is for a reaction between reactants A and B:
The order of the reaction with respect to A and B, respectively are:
| Rate mol \(L^{-1}s^{-1}\) |
[A] | [B] |
| \(2 \times10^{-3}\) | 0.1 M | 0.1 M |
| \(4 \times10^{-3}\) | 0.2 M | 0.1 M |
| \(1.6 \times10^{-2}\) | 0.2 M | 0.2 M |
| 1. | 1, 0 | 2. | 0, 1 |
| 3. | 1, 2 | 4. | 2, 1 |
Subtopic: Order, Molecularity and Mechanism |
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Level 1: 80%+
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