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

Which of the following is an incorrect expression for the rate of reaction?

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:
\(5 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{BrO}_3^{-}(\mathrm{aq})+6 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow 3 \mathrm{Br}_2(\mathrm{aq})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{l})\)

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 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 ) 

For a reaction, 2A + B → C + D, the following observations were recorded:

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. bar^1/2 min    
2. bar² min^–1   
3. bar^–1 min^–2  
4. bar^–1/2 min^–1

True statement among the following is:

$1.$ $6.67$ $\times {10}^{-2}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$
$2.$ $2.67$ $\times$ ${10}^{-4}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$ $$
$3.$ $4.67$ $\times$ ${10}^{-3}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$
$4.$ $4.27$ $\times$ ${10}^3$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$

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 ${\mathrm{N}}_2{\mathrm{O}}_5$ at that time will be: 

1. 1.732 mol L⁻¹

2. 3.0 mol L⁻¹

3. $1.02$ $\times$ ${10}^{-4}$ mol L⁻¹

4. $3.4$ $\times$ ${10}^5$ mol L⁻¹