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. | \(-\frac{d[A]}{2 d t}\) |
The following reaction was carried out at 300 K.
2SO2(g) + O2(g) → 2SO3(g)
The rate of formation of is related to the rate of disappearance of by the following expression:
1.
2.
3.
4. None of the above.
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. | \(\frac{\Delta\left[\mathrm{Br}^{-}\right]}{\Delta t}=6 \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t}\) |
A reaction is first-order with respect to A and second-order with respect to B. The concentration of B is increased three times. The new rate of the reaction would:
| 1. | Decrease 9 times | 2. | Increase 9 times |
| 3. | Increase 6 times | 4. | Decrease 6 times |
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
During the formation of ammonia by Haber's process N2 + 3H2 → 2NH3, the rate of appearance of NH3 was measured as 2.5 x 10-4 mol L-1 s-1. The rate of disappearance of H2 will be:
1. 2.5 x 10-4 mol L-1 s-1
2. 1.25 x 10-4 mol L-1 s-1
3. 3.75 x 10-4 mol L-1 s-1
4. 15.00 x 10-4 mol L-1 s-1
For the reaction, \(\mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3,\) if, \(\frac{d[NH_{3}]}{dt} \ = \ 2\times 10^{-4} \ mol \ L^{-1} \ s^{-1}\), the value of \(\frac{-d[H_{2}]}{dt}\) would be:
| 1. | \(3 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \) | 2. | \(4 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \) |
| 3. | \(6 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \) | 4. | \(1 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\) |
The rate constant of a particular reaction has the dimension of frequency. The order of the reaction is:
1. Zero.
2. First.
3. Second.
4. Fractional.
Which of the following statements about the order of reaction is incorrect?
| 1. | Order is not influenced by the stoichiometric coefficient of the reactants. |
| 2. | Order of reaction is the sum of power to the concentration terms of reactants to express the rate of reaction. |
| 3. | The order of reaction is always a whole number. |
| 4. | Order can be determined by experiments only. |
© 2024 GoodEd Technologies Pvt. Ltd.