Q. No.The results given in the below table were obtained during kinetic studies of the following reaction:
2A + B C + D
| Experiment | [A]/mol L-1 | [B]/mol L-1 | Initial rate/mol L-1 min-1 |
| I | 0.1 | 0.1 | 6.0010-3 |
| II | 0.1 | 0.2 | 2.4010-2 |
| III | 0.2 | 0.1 | 1.2010-2 |
| IV | X | 0.2 | 7.2010-2 |
| V | 0.3 | Y | 2.8810-1 |
X and Y in the given table are respectively :
1. 0.3, 0.4
2. 0.4, 0.3
3. 0.4, 0.4
4. 0.3, 0.3
For the reaction \(2 A+B \rightarrow C,\) the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is:
| [A] (mol L-1) | [B] (mol L-1) | Initial Rate (mol L-1 s-1) |
| 0.05 | 0.05 | 0.045 |
| 0.10 | 0.05 | 0.090 |
| 0.20 | 0.10 | 0.72 |
| 1. | \(\text { Rate }=\mathrm{k}[A][B]\) | 2. | \(\text { Rate }=\mathrm{k}[\mathrm{~A}][B]^2\) |
| 3. | \(\text { Rate }=\mathrm{k}[A]^2[B]^2\) | 4. | \(\text { Rate }=\mathrm{k}[A]^2[B]\) |
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.
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 |
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
A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will:
1. Remain unchanged
2. Triple
3. Increases by a factor of 4
4. Double
H2 gas is absorbed on the metal surface like gold, tungsten, etc. This follows ________ order reaction:
| 1. | Third | 2. | Second |
| 3. | Zero | 4. | First |
For the reaction system : \(2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)\), volume is suddenly reduced to half its value by increasing the pressure. If the reaction is of first order with respect to O2 and second order with respect to NO; the rate of reaction will:
1. Diminish to one -fourth of its initial value
2. Diminish to one-eighth of its initial value
3. Increase to eight times of its initial value
4. Increase to four times of its initial value
Find out the order of a reaction \(A + 2B\rightarrow C\) , if the rate is given by \(+\frac{d[C]}{d t}=k[A][B]\):
1. Three (3)
2. Two (2)
3. One (1)
4. Zero (0)
\(\mathrm{A} \xrightarrow{\mathrm{k}_1} \mathrm{~B} \xrightarrow{\mathrm{k}_2} \mathrm{C}\)
If net rate of formation of B is zero, what would be concentration of B in terms of concentration of A?
1. \(\mathrm{k}_1 \mathrm{k}_2[\mathrm{~A}] \)
2. \( \frac{k_1}{k_2}[A]\)
3. \( \left(k_1+k_2\right)[A] \)
4. \( \frac{k_2}{k_1}[A]\)
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