Q. No.
For the reaction, \(2 A+B \rightarrow 3 C+D\)
Which of the following is an incorrect expression for the rate of reaction?
| 1. | \(-\frac{d[C]}{{3} d t }\) | 2. | \(-\frac{d[B]}{d t} \) |
| 3. | \(\frac{d[D]}{d t} \) | 4. | \(-\frac{d[A]}{2 d t}\) |
For a general reaction A B, the plot of the concentration of A vs. time is given in the figure.
The slope of the curve will be:
| 1. | -k | 2. | -k/2 |
| 3. | -k2 | 4. | -k/3 |
The correct expression for the rate of reaction given below is:
\(5 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{BrO}_3^{-}(\mathrm{aq})+6 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow 3 \mathrm{Br}_2(\mathrm{aq})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{l})\)
| 1. | \(\frac{\Delta\left[B r^{-}\right]}{\Delta t}=5 \frac{\Delta\left[H^{+}\right]}{\Delta t} \) | 2. | \(\frac{\Delta\left[\mathrm{Br}^{-}\right]}{\Delta t}=\frac{6}{5} \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t} \) |
| 3. | \(\frac{\Delta[\mathrm{Br^-}]}{\Delta t}=\frac{5}{6} \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t} \) | 4. | \(\frac{\Delta\left[\mathrm{Br}^{-}\right]}{\Delta t}=6 \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t}\) |
For the reaction,
N2O5(g) → 2NO2(g) + \(\frac{1}{2}\)O2(g)
the value of the rate of disappearance of is given as . The rate of formation of is given respectively as:
1. 6.25 x 10-3 mol L-1s-1 and 6.25 x 10-3 mol L-1s-1
2. 1.25 x 10-2 mol L-1s-1 and 3.125 x 10-3 mol L-1s-1
3. 6.25 x 10-3 mol L-1s-1 and 3.125 x 10-3 mol L-1s-1
4. 1.25 x 10-2 mol L-1s-1 and 6.25 x 10-3 mol L-1s-1
The decomposition of NH3 on a platinum surface is a zero-order reaction. The rates of production of N2 and H2 will be respectively:
(given ; k = 2.5 × 10–4 mol–1 L s–1 )
| 1. | 2.5 × 10−4 mol L−1 s−1 and 5.5 × 10−4 mol L−1 s−1
|
| 2. | 2.5 × 10−4 mol L−1 s−1 and 7.5 × 10−4 mol L−1 s−1
|
| 3. | 1.5 × 10−4 mol L−1 s−1 and 4.5 × 10−4 mol L−1 s−1
|
| 4. | 0.5 × 10−4 mol L−1 s−1 and 3.5 × 10−4 mol L−1 s−1 |
For a reaction, 2A + B → C + D, the following observations were recorded:
| Experiment | [A]/mol L–1 | [B]/mol L–1 | Initial rate of formation of D/mol L–1 min–1 |
| I | 0.1 | 0.1 | 6.0 × 10–3 |
| II | 0.3 | 0.2 | 7.2 × 10–2 |
| III | 0.3 | 0.4 | 2.88 × 10–1 |
| IV | 0.4 | 0.1 | 2.40 × 10–2 |
The rate law applicable to the above mentioned reaction would be:
1. Rate = k[A]2[B]3
2. Rate = k[A][B]2
3. Rate = k[A]2[B]
4. Rate = k[A][B]
The rate equation of a reaction is expressed as, Rate = \(k(P_{CH_{3}OCH_{3}})^{\frac{3}{2}}\)
(Unit of rate = bar min–1)
The units of the rate constant will be:
1. bar1/2 min
2. bar2 min–1
3. bar–1 min–2
4. bar–1/2 min–1
True statement among the following is:
| 1. | The rate of a reaction decreases with the passage of time as the concentration of reactants decreases. |
| 2. | The rate of a reaction is the same at any time during the reaction. |
| 3. | The rate of a reaction is independent of temperature change. |
| 4. | The rate of a reaction decreases with an increase in the concentration of the reactants. |
| t/s | 0 | 30 | 60 | 90 |
| [Ester]/mol L–1 | 0.55 | 0.31 | 0.17 | 0.085 |
If at a given instant, for the reaction 2N2O5 → 4NO2 + O2 rate and rate constant are 1.02 × 10-4 and 3.4 × 10-5 sec -1 respectively, then the concentration of at that time will be:
1. 1.732
2. 3.0
3.
4.
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