Q. No.| Column I: |
Column II: |
||
| (A) | Zero order | (i) | \(k=Ae^{-E_a/RT}\) |
| (B) | First order | (ii) |  |
| (C) | Endothermic reaction | (iii) | \( k=\frac{2.303}{t} \log \frac{[A]_0}{[A]} \) |
| (D) | Arrhenius equation | (iv) | \( k=\frac{1}{t}\left([A]_0-[A]\right)\) |
1. (A) →(iv), (B)→(iii), (C) →(ii), (D)→ (i)
2. (A) →(i), (B)→(ii), (C) →(iii), (D)→ (iv)
3. (A) →(ii), (B)→(iii), (C) →(iv), (D)→ (i)
4. (A) →(iii), (B)→(iv), (C) →(i), (D)→ (ii)
1. 50 min.
2. 60 min
3. 40 min
4. 30 min
Which of the following is the mass of a radioisotope remaining undecayed after 24 hours, if its half-life is 4 hours and the initial mass is 200 g?
1. 1.042 g
2. 2.084 g
3. 3.125 g
4. 4.167 g
Which of the following represents the factor by which the rate of a zero-order reaction increases when the temperature is raised from 10°C to 100°C, if the rate doubles for every 10°C rise in temperature?
1. 256 times
2. 512 times
3. 64 times
4. 128 times
| 1. | Inversion of cane sugar |
| 2. | Radioactive decay |
| 3. | Hydrogenation of ethene |
| 4. | Decomposition of gaseous ammonia on a hot platinum surface at high pressure |
| 1. |  |
2. |  |
| 3. |  |
4. |  |
The correct statements among the following regarding a balanced chemical equation of an elementary reaction are-
| a. | Order is the same as molecularity. |
| b. | Order is less than the molecularity. |
| c. | Order is greater than molecularity. |
| d. | Molecularity can never be zero. |
1. (a, b)
2. (b, c)
3. (c, d)
4. (a, d)
1. 4
2. 6
3. 3
4. 5
A first-order reaction has a rate constant of 2.303 × 10¯3 s¯1. The time required for 40 g of this reactant to reduce to 10 g will be
[Given that ]
| 1. | 230.3 s | 2. | 301 s |
| 3. | 2000 s | 4. | 602 s |
For a first order reaction A→B, the reaction rate at reactant concentration of 0.01M is found to be
2.0×10-5 mol L-1s-1. The half-life period of the reaction is:
| 1. | 220 s | 2. | 30 s |
| 3. | 300 s | 4. | 347 s |
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