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 |
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
H2 gas is absorbed on the metal surface like gold, tungsten, etc. This follows ________ order reaction:
1. Third
2. Second
3. Zero
4. 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
1. | –1.5 | 2. | 1.5 |
3. | 0.5 | 4. | 2.5 |
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
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 |
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
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.
2.
3.
4.