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
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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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


 
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, \(2 \mathrm{Na}+\mathrm{Cl}_2\rightarrow2 \mathrm{NaCl}\) 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 gold, tungsten, etc. 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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Which of the following curves represents a first-order reaction?

1. 
2. 
3. 
4. 
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.  \(3.6\times10^{30}~s^{-1}\)
Subtopic:  Arrhenius Equation |
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