# The rate equation for the reaction 2A+B→C is found to be: rate = k [A] [B] The correct statement in relation to this reaction is that the: 1. Unit of k must be s-1 2. t1/2 is a constant 3. Rate of formation of C is twice the rate of disappearance of A 4. Value of k is independent of the initial concentrations of A and B

Subtopic:  Definition, Rate Constant, Rate Law |
54%
From NCERT
Please attempt this question first.
Hints
Please attempt this question first.

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%
From NCERT
Please attempt this question first.
Hints
Please attempt this question first.

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 |
68%
From NCERT
Please attempt this question first.
Hints
Please attempt this question first.

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%
From NCERT
Please attempt this question first.
Hints
Please attempt this question first.

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 |
From NCERT
To view explanation, please take trial in the course.
NEET 2025 - Target Batch
Hints
To view explanation, please take trial in the course.
NEET 2025 - Target Batch

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 |
77%
From NCERT
Please attempt this question first.
Hints
Please attempt this question first.

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
Please attempt this question first.
Hints
Please attempt this question first.

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 |
70%
From NCERT
Please attempt this question first.
Hints
Please attempt this question first.

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%
From NCERT
Please attempt this question first.
Hints
Please attempt this question first.

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 |
76%
From NCERT
Please attempt this question first.
Hints
Please attempt this question first.