Q. No.Mechanism is expressed in three steps:
Step -1 : \(\mathrm{A} \rightarrow \mathrm{~B}: \Delta \mathrm{H}=+\mathrm{ve}\)
Step -2 : \( B \rightarrow C: \Delta H=-\mathrm{ve} \)
Step -3 : \( C \rightarrow D: \Delta H=-\mathrm{ve}\)
1.
2. 
3.
4. 
\(\mathrm{A} \xrightarrow{\mathrm{k}_1} \mathrm{~B} \xrightarrow{\mathrm{k}_2} \mathrm{C}\)
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. \( \frac{k_2}{k_1}[A]\)
\(\mathrm{N}_2 \mathrm{O}_4 \rightarrow 2 \mathrm{NO}_2\)
Initial conc. of \(\text{N}_2\text{O}_4=3\text{M}\)
If the concentration of \(\text{N}_2\text{O}_4\) is 2.75 M, after 30 sec., then find out the rate of formation of \(\text{NO}_2\) during this interval in \(\text {mol} ~ \text{lit}^{-1}~\text{min}^{-1}\).
1. 4
2. 1
3. 6
4. 0
The rate law for a reaction is rate = k[A]²[B]. If the concentrations of both A and B are doubled, the rate becomes x times the original rate, and the overall order of the reaction is y. The value of (x + y) is:
| 1. | 11 | 2. | 87 |
| 3. | 67 | 4. | 20 |
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.
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)
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
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