Based on the graph below, the average rate of reaction will be: 

1.  \(\frac{[R_{2}]-[R_{1}]}{t_{2}-t_{1}}\)
2.  \(-(\frac{[R_{2}]-[R_{1}]}{t_{2}-t_{1}})\)
3.  \(\frac{[R_{2}]}{t_{2}}\)
4.  \(-(\frac{[R_{1}]-[R_{2}]}{t_{2}-t_{1}})\)

Match the items in Column I with Column II:

Codes:

Consider the following graph:
      

The instantaneous rate of reaction at t = 600 sec will be:

$1. - 4.75$ $\times {10}^{-4}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$
$2.$ $5.75\times {10}^{-5}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$
$3.$ $$ $6.75\times {10}^{-6}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$
$4.$ $-6.75\times {10}^{-6}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$

In the following reaction: xA →  yB

$\log \left(-\frac{d\left[A\right]}{d\mathrm{t }}\right)=$ $\log$ $\left(\frac{d\left[B\right]}{dt}\right)$ $+$ $0.3$ 

where the -ve sign indicates the rate of disappearance of the reactant. Then, x : y equals:

A gaseous reaction A₂(g) → B(g) + $\frac{1}{2}C$(g) shows increase in pressure from 100 mm to 120 mm in 5 minutes. The rate of disappearance of A₂ will be : 

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,

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

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 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:

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

An incorrect expression for the rate of reaction is: