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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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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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. $$Rate = K [A]^3[B]^2$$
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
Subtopic:  Order, Molecularity and Mechanism |
68%
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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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The time for the half-life period of a certain reaction A → Products is 1 hour. When the initial concentration of the reactant 'A' is 2.0 mol L-1, the time taken for its concentration to come from 0.50 to 0.25 mol L-1,if it is a zero-order reaction, is:

1. 1h

2. 4 h

3. 0.5 h

4. 0.25 h

Subtopic:  Order, Molecularity and Mechanism |
66%
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Consider the reaction, 2A + B → Products.
When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:

1. L mol–1 s–1

2. no unit

3. mol L–1s–1

4. s–1

Subtopic:  Order, Molecularity and Mechanism |
From NCERT
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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 non – stoichiometry reaction 2A + B → C + D, the following kinetic data were obtained in three separate experiments (all at 298 K).

 Initial Concentration (A) Initial Concentration (B) Initial rate of formation of C (mol L– S–) 0.1 M 0.1 M 0.2 M 0.1 M 0.2 M 0.1 M 1.2 × 10–3 1.2 × 10–3 2.4 × 10–3

The rate law for the formation of C is:

1. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}{\right]}^{2}\left[\mathrm{B}\right]$

2. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right]\left[\mathrm{B}{\right]}^{2}$

3. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right]$

4. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right]\left[\mathrm{B}\right]$

Subtopic:  Order, Molecularity and Mechanism |
77%
From NCERT