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Q. No.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 |
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NEET 2023 - Target Batch - Aryan Raj Singh
| Assertion (A): | For an endothermic reaction, the potential energy of the reactant is more than the potential energy of the product. |
| Reason (R): | Reactant molecules before converting to product form an activated complex that has lower energy than reactants as well as the products. |
| 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 but (R) is false. |
| 4. | Both (A) and (R) are false. |
Subtopic: Arrhenius Equation |
65%
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The plot of concentration of a reactant vs. time for a chemical reaction is shown below:
The order of this reaction with respect to the reactant is:
1. 0
2. 1
3. 2
4. not possible to determine from this plot
The order of this reaction with respect to the reactant is:
1. 0
2. 1
3. 2
4. not possible to determine from this plot
Subtopic: Order, Molecularity and Mechanism |
68%
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Given the reaction, \(A + B \rightarrow Products,\) , when concentration of A is fixed and concentration of B is increased 3 times then rate of reaction increases 27 times. Now, when the concentration of A and B both are doubled, then the rate of reaction increases 8 times. The rate law for the reaction will be
1. \(Rate = K [A]^2[B] \)
2. \(Rate = K [B]^3 \)
3. \(Rate = K [A]^3[B] \)
4. \(Rate = K [A]^3[B]^2\)
1. \(Rate = K [A]^2[B] \)
2. \(Rate = K [B]^3 \)
3. \(Rate = K [A]^3[B] \)
4. \(Rate = K [A]^3[B]^2\)
Subtopic: Order, Molecularity and Mechanism |
83%
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The rate constant, the activation energy and the Arrhenius parameter of a chemical reaction at \(25^{\circ}C\) are \(3\times10^{-4}~s^{-1},104.4~kJ~mol^{-1}\) and \(6\times10^{14}~s^{-1}\) respectively. The value of the rate constant as \(T\rightarrow\infty\) is
1. \(2\times10^{18}~s^{-1}\)
2. \(6\times10^{14}~s^{-1}\)
3. \(\infty\)
4. \(3.6\times10^{30}~s^{-1}\)
1. \(2\times10^{18}~s^{-1}\)
2. \(6\times10^{14}~s^{-1}\)
3. \(\infty\)
4. \(3.6\times10^{30}~s^{-1}\)
Subtopic: Arrhenius Equation |
78%
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Subtopic: First Order Reaction Kinetics |
85%
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Which of the following statements is not true for the rate constant, k?
| 1. | large value of k indicates fast reactions. |
| 2. | The value of k is independent of the concentration of reactants |
| 3. | The value of k is independent of the concentration of products |
| 4. | The value of the rate constant, k, as the name suggests is always constant for a particular reaction at all temperatures. |
Subtopic: Arrhenius Equation |
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Example(s) of a pseudo-unimolecular reaction among the following is/are:
| 1. | \(\small{CH_3COOC_2H_5 + NaOH \rightarrow CH_3COONa + C_2H_5OH}\) |
| 2. | \(\small{CH_3COOC_2H_5 + H_2O \xrightarrow{H^+} CH_3COOH + C_2H_5OH}\) |
| 3. | \(C_{12}H_{22}O_{11}+ H_2O \xrightarrow{H^+} C_6H_{12}O_6+ C_6H_{12}O_6\\ (cane~ sugar)~~~~~~~~~~~~~~~~(glucose)~~~~~(Fructose)\) |
| 4. | Both 2 and 3 |
Subtopic: Order, Molecularity and Mechanism |
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For the reaction, A + B → Products
The rate law and unit of rate constant respectively, are:
| Experiment | [A] | [B] | Rate (mole litre-1 min-1) |
| 1. | 0.01 | 0.01 | 2 × 10-4 |
| 2. | 0.02 | 0.01 | 4 × 10-4 |
| 3. | 0.01 | 0.02 | 8 × 10-4 |
| 1. | Rate = K [A]2 [B] and litre2 mole-2 min-1 |
| 2. | Rate = K [A]3 and litre2 mole-2 min-1 |
| 3. | Rate = K [A] [B]2 and litre mole-1 min-1 |
| 4. | Rate = K [A] [B]2 and litre2 mole-2 min-1 |
Subtopic: Order, Molecularity and Mechanism |
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For a reaction, A + B → Product; the rate law is given by, r=k[A]1/2[B]2. The order of the reaction is:
| 1. | -1.5 | 2. | 1.5 |
| 3. | 0.5 | 4. | 2.5 |
Subtopic: Order, Molecularity and Mechanism |
77%
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