Which one of the following statements for the order of a reaction is incorrect?

1. Order is not influenced by stiochiometric coefficient of the reactants.

2. Order of reaction is sum of power to the concentration terms of reactants to express the rate of reaction.

3. Order of reaction is always whole number.

4. Order can be determined only experimentally.

 

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

For an endothermic reaction, energy of activation is E_a and enthalpy of reaction is $∆$H (both of these in kJ/mol). Minimum value of E_a will be

1. Less than $∆$H

2. Equal to $∆$H

3. More than $∆$H

4. Equal to zero

During the kinetic study of the reaction, 2A + B → C + D, the following results were obtained:

Based on the above data, the correct rate law is:
1.  Rate=k[A]²[B]

2.  Rate=k[A][B]

3.  Rate=k[A]²[B]²

4.  Rate=k[A][B]²

Half-life period of a first order reaction is 1386s. The specific rate constant of the reaction

is

1. 5.0 x 10^-3s^-1

2. 0.5 x 10^-2s^-1

3. 0.5 x 10^-3s^-1

4. 5.0 x 10^-2s^-1

For the reaction A+B $\to$products, it is observed that
 

The rate of this reaction is, given by

1. rate = k[A]²[B]

2. rate = k[A][B]²

3. rate = k[A]²[B]²

4. rate = k[A][B]

For the reaction, N₂ + 3H₂ $\to$2NH₃, if d[NH₃]/dt = 2x10^-4 mol L^-1s^-1, the value of -

d[H₂]/dt would be 

1. 3x10^-4 mol L^-1s^-1

2. 4x10^-4 mol L^-1s^-1

3. 6x10^-4 mol L^-1s^-1

4. 1x10^-4 mol L^-1s^-1

In the reaction, BrO^-₃(aq) + 5Br^-(aq) + 6H⁺ $\to$3Br₂(l) + 2H₂O(l)

The rate of appearance of bromine (Br₂) is related to rate of disappearance of bromide

ions as following 

1. d[Br₂]/dt = -(3/5)d[Br^-]/dt

2. d[Br₂]/dt = (5/3)d[Br^-]/dt

3. d[Br₂]/dt = -(5/3)d[Br^-]/dt

4. d[Br₂]/dt = (3/5)d[Br^-]/dt

The rate constants k₁ and k₂ for two different reactions are 10¹⁶ e^-2000/T and 10¹⁵ e^-1000/T  , respectively. The temperature at which k₁=k₂ is:

(1) 1000 K

(2) $\frac{2000}{2.303}\mathrm{K}$

(3) 2000K

(4) $\frac{1000}{2.303}\mathrm{K}$

The bromination of acetone that occurs in acid solution is represented by this equation.

${\mathrm{CH}}_3{\mathrm{COCH}}_3\left(\mathrm{aq}\right) + {\mathrm{Br}}_2\left(\mathrm{aq}\right) \stackrel{ }{\to }{\mathrm{CH}}_3{\mathrm{COCH}}_2\mathrm{Br}\left(\mathrm{aq}\right) + {\mathrm{Br}}^{-}\left(\mathrm{aq}\right)$

These kinetic data were obtained for given reaction concentrations. 

                   Initial concentrations, M

  $\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right]$                $\left[{\mathrm{Br}}_2\right]$         $\left[{\mathrm{H}}^{+}\right]$

       0.30                        0.05           0.05

       0.30                        0.10           0.05

       0.30                        0.10           0.10

       0.40                        0.05           0.20

Initial rate, disappearance of Br₂, Ms^-1

                        5.7X10^-5

                        5.7X10^-5

                        1.2X10^-4

                        3.1X10^-4

Based on these data, the rate equation is

1. Rate = k [CH₃COCH₃] [H⁺]

2. Rate = k [CH=COCH₃][Br₂]

3. Rate = k [CH₃COCH₃][Br₂][H⁺]²

4. Rate = k [CH₃COCH₃][Br₂][H⁺]