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Q. No.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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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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The rate constants of a reaction at 500K is 0.02s–1 . The values of Ea is 18.230 kJ. The value of A is-
1. 1.61
2. 1.41
3. 1.81
4. 1.21
1. 1.61
2. 1.41
3. 1.81
4. 1.21
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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The elementary step of the reaction, is found to follow 3rd order kinetics. Its molecularity is:
1. 1
2. 2
3. 3
4. 4
Subtopic: Order, Molecularity and Mechanism |
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H2 gas is absorbed on the metal surface like tungsten. This follows ________ order reaction:
1. Third
2. Second
3. Zero
4. First
Subtopic: Order, Molecularity and Mechanism |
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Half-life of substance A following first order kinetics is 5 days. Starting with 100g of A, the amount left after 15 days will be:
1. 25 g
2. 50 g
3. 12.5 g
4. 6.25 g
Subtopic: First Order Reaction Kinetics |
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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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