Q. No.A first-order reaction is 50 % completed in 1.26 × 1014 s.
The time required for 100 % completion of the reaction will be:
1. 1.26 × 1015 s
2. 2.52 × 1014 s
3. 2.52 × 1028 s
4. Infinite
Compounds A and B react according to the following chemical equation.
A(g) + 2B(g) 2C(g)
The concentration of either A or B was changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. The following results were obtained. Choose the correct option for the rate equations for this reaction.
| Experiment | Initial concentration of [A]/mol L–1 |
Initial concentration of [B]/moI L–1 |
Initial rate (mol L–1 s–1) |
| 1. 2. 3. |
0.30 0.30 0.60 |
0.30 0.60 0.30 |
0.10 0.40 0.20 |
2.
3.
4.
An incorrect statement regarding a catalyst is:
| 1. | It catalyzes the forward and backward reactions to the same extent. |
| 2. | It alters the Gibbs free energy of the reaction. |
| 3. | It is a substance that does not change the equilibrium constant of a reaction. |
| 4. | It provides an alternate mechanism by reducing activation energy between reactants and products. |
Consider the reaction AB. The concentration of both the reactant and the product varies exponentially with time.
The graph that accurately depicts how reactant and product concentrations change with time is:
| 1. |  |
2. |  |
| 3. |  |
4. |  |
The graphs that represent a zero-order reaction are:
| (a) |  |
(b) |  |
| (c) |  |
(d) |  |
| 1. | a and b | 2. | b and c |
| 3. | c and d | 4. | a and d |
The correct graphical representation of first-order reaction is:
| (a) |  |
(b) |  |
| (c) |  |
(d) |  |
| 1. | (a) and (b) | 2. | (b) and (c) |
| 3. | (c) and (d) | 4. | (a) and (d) |
Match the graph given in Column I with the order of reaction given in Column II.
More than one item in Column I may be linked to the same item in Column II:
| Column I | Column II | ||
| (i) |  |
(a) | 1st order |
| (ii) |  |
(b) | Zero order |
| (iii) |  |
||
| (iv) |  |
||
| (i) | (ii) | (iii) | (iv) | |
| 1. | (a) | (b) | (a) | (b) |
| 2. | (a) | (b) | (b) | (a) |
| 3. | (a) | (a) | (b) | (b) |
| 4. | (b) | (b) | (a) | (a) |
|
Column I
(Thermodynamic/Kinetic Principle)
|
Column II
(Impact on Reaction Dynamics)
|
||
| A. | Catalyst alters the rate of reaction | 1. | Proper orientation is not always there |
| B. | 2. | By lowering the activation energy | |
| C. | Energetically favorable reactions are sometimes slow | 3. | Total probability is one |
| D. | The area under the Maxwell-Boltzmann curve is constant | 4. | Refers to the fraction of molecules with energy equal to or greater than the activation energy |
Codes:
| A | B | C | D | |
| 1. | 2 | 4 | 1 | 3 |
| 2. | 3 | 1 | 4 | 2 |
| 3. | 1 | 4 | 3 | 2 |
| 4. | 3 | 4 | 1 | 2 |
Match the items in Column I with Column II:
| Column I | Column II |
| A. Diamond to graphite conversion | 1. Short interval of time |
| B. Instantaneous rate | 2. Ordinarily rate of conversion is imperceptible |
| C. Average rate | 3. Long duration of time |
Codes:
| A | B | C | |
| 1. | 2 | 1 | 3 |
| 2. | 1 | 2 | 3 |
| 3. | 3 | 2 | 1 |
| 4. | 1 | 3 | 2 |
Match the items of Column-I with items of Column-II:
| Column-I (Concepts Related to Chemical Kinetics) |
Column-II (Related Terms) |
||
| A. | Mathematical expression for the rate of reaction | I. | Rate constant |
| B. | Rate of reaction for zero-order reaction is equal to | II. | Rate law |
| C. | Units of rate constant for zero-order reaction is same as that of | III. | Order of slowest step |
| D. | Order of a complex reaction is determined by | IV. | Rate of reaction |
Codes:
| A | B | C | D | |
| 1. | III | IV | I | II |
| 2. | I | II | III | IV |
| 3. | II | I | IV | III |
| 4. | IV | I | III | II |
© 2026 GoodEd Technologies Pvt. Ltd.