For the reaction, \(2 A+B \rightarrow 3 C+D\)

An incorrect expression for the rate of reaction is:

The following reaction was carried out at 300 K.

2SO₂(g)  +  O₂(g) →  2SO₃(g)

The rate of formation of $S{O}_3$ is related to the rate of disappearance of $O_2$  by the following expression:

1. $-\frac{∆\left[O_2\right]}{∆t}=+\frac{1}{2}\frac{∆\left[S{O}_3\right]}{∆t}$                           

2. $-\frac{∆\left[O_2\right]}{∆t}=\frac{∆\left[S{O}_3\right]}{∆t}$

3. $-\frac{∆\left[O_2\right]}{∆t}=-\frac{1}{2}\frac{∆\left[S{O}_3\right]}{∆t}$                           

4. None of the above.

For a general reaction A $\to$ B, the plot of the concentration of A vs. time is given in the figure.
 

The slope of the curve will be:

The correct expression for the rate of reaction given below is:
\(5 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{BrO}_3^{-}(\mathrm{aq})+6 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow 3 \mathrm{Br}_2(\mathrm{aq})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{l})\)

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:

For the reaction,

N₂O₅(g) → 2NO₂(g) + \(\frac{1}{2}\)O₂(g)

the value of the rate of disappearance of ${\mathrm{N}}_2{\mathrm{O}}_5$ is given as $6.\mathrm{25 }\times {10}^{-3}$ $mol$ $L^{-1}{s}^{-1}$. The rate of formation of $N{O}_2$ $and$ $O_2$ 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$\mathrm{}{\mathrm{}}^{}$

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:

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.

The incorrect statement regarding the order of reaction is: