Q. No.Match List-I with List-II:
Choose the correct answer from the options given below:
| List-I (Order of reaction) | List-II (Unit of rate constant) | ||
| A. | Zero order | I. | \(\mathrm{mol}^{-1} \mathrm{~L} \mathrm{~s}^{-1}\) |
| B. | First order | II. | \(\mathrm{mol}^{-2} \mathrm{~L}^2 \mathrm{~s}^{-1}\) |
| C. | Second order | III. | \(\mathrm {s}^{-1}\) |
| D. | Third order | IV. | \(\mathrm{mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\) |
Choose the correct answer from the options given below:
| 1. | A-IV, B-III, C-II, D-I |
| 2. | A-I, B-II, C-III, D-IV |
| 3. | A-IV, B-III, C-I, D-II |
| 4. | A-IV, B-II, C-I, D-III |
Subtopic: Definition, Rate Constant, Rate Law | First Order Reaction Kinetics |
74%
Level 2: 60%+
NEET - 2026
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For a certain reaction R → Product, the plot of concentration [R] vs time has a negative slope as shown. The order of reaction is :
1. 0
2. 1
3. 2
4. 2.5
1. 0
2. 1
3. 2
4. 2.5
Subtopic: Definition, Rate Constant, Rate Law | Order, Molecularity and Mechanism |
67%
Level 2: 60%+
NEET - 2026
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Which of the following expression is correct for the reaction given below?
\(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)
\(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)
| 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 |
89%
Level 1: 80%+
NEET - 2024
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For a reaction \(3A \rightarrow 2B\)
The average rate of appearance of B is given by \(\Delta [B] \over \Delta t\).
The correct relation between the average rate of appearance of B with the average rate of disappearance of A is:
The average rate of appearance of B is given by \(\Delta [B] \over \Delta t\).
The correct relation between the average rate of appearance of B with the average rate of disappearance of A is:
| 1. | \(-\Delta [A] \over \Delta t\) | 2. | \(-3\Delta [A] \over 2\Delta t\) |
| 3. | \(-2\Delta [A] \over 3\Delta t\) | 4. | \(\Delta [A] \over \Delta t\) |
Subtopic: Definition, Rate Constant, Rate Law |
81%
Level 1: 80%+
NEET - 2023
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For the reaction, 2A → B, rates= k[A]2. If the concentration of reactant is doubled, then the:
| (a) | rate of reaction will be doubled. |
| (b) | rate constant will remain unchanged, however rate of reaction is directly proportional to the rate constant. |
| (c) | rate constant will change since the rate of reaction and rate constant are directly proportional to each other. |
| (d) | rate of reaction will increase by four times. |
Identify the set of correct statements & choose the correct answer from the options given below:
| 1. | (a) and (c) only | 2. | (a) and (b) only |
| 3. | (b) and (d) only | 4. | (c) and (d) only |
Subtopic: Definition, Rate Constant, Rate Law |
69%
Level 2: 60%+
NEET - 2022
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For a chemical reaction, 4A + 3B → 6C + 9D
rate of formation of C is 6 × 10–2 mol L–1 s–1 and rate of disappearance of A is 4 × 10–2 mol L–1 s–1. The rate of reaction and amount of B consumed in interval of 10 seconds, respectively will be:
rate of formation of C is 6 × 10–2 mol L–1 s–1 and rate of disappearance of A is 4 × 10–2 mol L–1 s–1. The rate of reaction and amount of B consumed in interval of 10 seconds, respectively will be:
| 1. | 1 × 10–2 mol L–1 s–1 and 30 × 10–2 mol L–1 |
| 2. | 10 × 10–2 mol L–1 s–1 and 10 × 10–2 mol L–1 |
| 3. | 1 × 10–2 mol L–1 s–1 and 10 × 10–2 mol L–1 |
| 4. | 10 × 10–2 mol L–1 s–1 and 30 × 10–2 mol L–1 |
Subtopic: Definition, Rate Constant, Rate Law |
71%
Level 2: 60%+
NEET - 2022
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For the chemical reaction ) the correct option is:
| 1. | \(3\frac {d[H_2]} {dt} = 2 \frac {d[NH_3]} {dt} \) | 2. | \(-\frac {1} {3}\frac {d[H_2]} {dt} = -\frac {1} {2} \frac {d[NH_3]} {dt} \) |
| 3. | \(- \frac{d \left[N_{2}\right]}{dt} = 2 \frac{d [NH_{3}]}{dt}\) | 4. | \(- \frac{d \left[N_{2}\right]}{dt} = \frac{1}{2} \frac{d [NH_{3}]}{dt}\) |
Subtopic: Definition, Rate Constant, Rate Law |
83%
Level 1: 80%+
NEET - 2019
Hints
The correct statement among the following is:
| 1. | the rate of a first-order reaction does not depend on reactant concentration; the rate of a second-order reaction does depend on reactant concentrations. |
| 2. | the half-life of a first-order reaction does not depend on [A]o; the half-life of a second-order reaction does depend on [A]0 |
| 3. | a first-order reaction can be catalyzed; a second-order reaction cannot be catalyzed. |
| 4. | the rate of a first-order reaction does depend on reactant concentrations; the rate of a second-order reaction does not depend on reactant concentrations |
Subtopic: Definition, Rate Constant, Rate Law |
78%
Level 2: 60%+
NEET - 2018
Hints
Which quantity is altered when a catalyst is introduced during a chemical reaction?
| 1. | Internal energy | 2. | Enthalpy |
| 3. | Activation energy | 4. | Entropy |
Subtopic: Definition, Rate Constant, Rate Law |
94%
Level 1: 80%+
NEET - 2016
Hints
In a reaction, A + B → Product, the rate is doubled when the concentration of B is doubled, and the rate increases by a factor of 8, when the concentrations of both the reactants (A and B) are doubled. The rate law for the reaction can be written as:
1. Rate = k[A][B]2
2. Rate = k[A]2[B]2
3. Rate = k[A][B]
4. Rate = k[A]2[B]
Subtopic: Definition, Rate Constant, Rate Law |
78%
Level 2: 60%+
AIPMT - 2012
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