A reaction having equal energies of activation for forward and reverse reactions has

1. $∆$S = 0

2. $∆$G = 0

3. $∆$H = 0

4. $∆$H = $∆$G = $∆$S = 0

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

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]

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⁺]

In a first order reaction A $\stackrel{ }{\to }$ B, if k is rate constant and initial concentration of the reactant A is 0.5 M then the half-life is :

(1) $\frac{0.693}{0.5k}$

(2) $\frac{\log 2}{k}$

(3) $\frac{\log 2}{k\sqrt{0.5}}$

(4) $\frac{\ln 2}{k}$

If a first-order reaction reaches 60% completion within 60 minutes, approximately how much time would it take for the same reaction to reach 50% completion? (log 4=0.60, log 5=0.69)

1. 50 min

2. 45 min

3. 60 min

4. 30 min