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Q. No.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 |
90%
Level 1: 80%+
NEET - 2024
Hints
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 |
70%
Level 2: 60%+
NEET - 2022
Hints
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 |
70%
Level 2: 60%+
NEET - 2022
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 |
93%
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
Hints
Rate constants of a reaction at 500 K and 700 K are 0.04 \(s^{-1}\) and 0.14 \(s^{-1}\) respectively, then the activation energy of the reaction is:
[Given: log 3.5 = 0.5441, R = \(8.31 \text J\text K^{-1} \text{mol}^{-1}\) ]
1. 18231 J
2. 18500 J
3. 18219 J
4. 18030 J
[Given: log 3.5 = 0.5441, R = \(8.31 \text J\text K^{-1} \text{mol}^{-1}\) ]
1. 18231 J
2. 18500 J
3. 18219 J
4. 18030 J
Subtopic: Arrhenius Equation |
51%
Level 3: 35%-60%
NEET - 2024
Hints
Which of the following plot represents the variation of \(ln ~k\) versus \(\frac 1{T}\) according to the Arrhenius equation?
| 1. |  |
2. |  |
| 3. |  |
4. |  |
Subtopic: Arrhenius Equation |
85%
Level 1: 80%+
NEET - 2024
Hints
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 |
57%
Level 3: 35%-60%
NEET - 2024
Hints
Given below are two statements:
| Assertion (A): | A reaction can have zero activation energy. |
| Reason (R): | The minimum amount of energy required by reactant molecules so that their energy becomes equal to threshold value, is called activation energy. |
| 1. | (A) is False but (R) is True. |
| 2. | Both (A) and (R) are True and (R) is the correct explanation of (A) |
| 3. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
| 4. | (A) is True but (R) is False. |
Subtopic: Arrhenius Equation |
Level 4: Below 35%
NEET - 2023
Hints
The slope of Arrhenius Plot (ln k v/s ) of the first-order reaction is . The value of Ea of the reaction is:
[Given R = 8.314 JK–1 mol–1]
| 1. | 166 kJ mol–1 | 2. | –83 kJ mol–1 |
| 3. | 41.5 kJ mol–1 | 4. | 83.0 kJ mol–1 |
Subtopic: Arrhenius Equation |
77%
Level 2: 60%+
NEET - 2021
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