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Q. No.For the reaction, A + B → Products
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
The rate law and unit of rate constant respectively, are:
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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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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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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Subtopic: First Order Reaction Kinetics |
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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 |
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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 |
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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 |
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| 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 |
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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 |
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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 |
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