# 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 |
81%
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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 |
86%
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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 |
71%
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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.  $$3.6\times10^{30}~s^{-1}$$