Q. No.CH3COOC2H5 + H2O \(\xrightarrow[]{H^{+}}\) CH3COOH + C2H2OH
Ethyl acetate Acetic acid Ethyl alcohol
1. Pseudo-first-order reaction
2. First-order reaction
3. Second order reaction
4. Third-order reaction
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 | 1. | Rate constant |
| B. | Rate of reaction for zero-order reaction is equal to | 2. | Rate law |
| C. | Units of rate constant for zero-order reaction is same as that of | 3. | Order of slowest step |
| D. | Order of a complex reaction is determined by | 4. | Rate of reaction |
Codes:
| A | B | C | D | |
| 1. | 3 | 4 | 1 | 2 |
| 2. | 1 | 2 | 3 | 4 |
| 3. | 2 | 1 | 4 | 3 |
| 4. | 4 | 1 | 3 | 2 |
When the initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction will be:
1. 0
2. 1
3. 1.5
4. 2
The kinetic data for the reaction: 2A + B2 → 2AB are as given below
| [A]/mol L-1 | [B2]/mol L-1 | Rate/mol L-1s-1 |
| 0.5 | 1.0 | 2.5 × 10-3 |
| 1.0 | 1.0 | 5.0 × 10-3 |
| 0.5 | 2.0 | 1 × 10-2 |
The order of reaction with respect to A and B2 is, respectively:
| 1. | 1 and 2 | 2. | 2 and 1 |
| 3. | 1 and 1 | 4. | 2 and 2 |
| Assertion (A): | Order and molecularity are the same. |
| Reason (R): | Order is determined experimentally, and molecularity is the sum of the stoichiometric coefficient of the rate-determining the elementary step. |
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
| 3. | (A) is True but (R) is False. |
| 4. | (A) is False but (R) is True. |
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) |
Select the correct option based on statements below:
| Assertion (A): | For elementary reactions, the law of mass action and the rate of law expression are generally the same. |
| Reason (R): | The molecularity of an elementary reaction is always one. |
| 1. | Both (A) and (R) are true and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are true but (R) is not the correct explanation of (A). |
| 3. | (A) is true but (R) is false. |
| 4. | Both (A) and (R) are false. |
For a given reaction the concentration of the reactant plotted against time gave a straight line with negative slope.
The order of the reaction will be:
1. 3
2. 2
3. 1
4. 0
A reaction A2 + B2 2AB occurs by the following mechanism:
A2 A + A .....(slow)
A + B2 AB + B .....(fast)
A + B AB .....(fast)
Its order would be:
1. 3/2
2. 1
3. 0
4. 2
The mechanism of a hypothetical reaction
X2 + Y2 → 2XY is given below:
(i) X2 → X + X (Fast)
(ii) X + Y2 ⇄ XY + Y (slow)
(iii) X + Y → XY (Fast)
The overall order of the reaction will be:
1. 2
2. 0
3. 1.5
4. 1
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