Order Molecularity And Mechanism

For the reaction,
${\mathrm{N}}_2{\mathrm{O}}_5\left(\mathrm{g}\right)\to 2{\mathrm{NO}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)$
the value of rate of disappearance of N₂O₅ is given as 6.25 x 10^-3mol L^-1s^-1.The rate of formation of NO₂ and O₂ is given respectively as:

1.	6.25 \times 10-3 mol L-1s-1 and 6.25 \times 10-3 mol L-1s-1.
2.	1.25 \times 10-2 mol L-1s-1 and 3.125 \times 10-3 mol L-1s-1.
3.	6.25 \times 10-3 mol L-1s-1 and 3.125 \times 10-3 mol L-1s-1.
4.	1.25 \times 10-2 mol L-1s-1 and 6.25 \times 10-3 mol L-1s-1.

The rate Constant of reaction A → B is 0.6 \times 10^–3 . If the Concentration of A is 5M, then the concentration of B after 20 min is:

1. 1.08M

2. 3.60M

3. 0.36M

4. 0.72M

The mechanism of a hypothetical reaction X₂ + Y₂ → 2XY is given below:
(i) X₂ → X + X (Fast)
(ii) X + Y₂ ⇄ XY + Y (slow)
(iii) X + Y → XY (Fast)

The overall order of the reaction will be:

1. 2

2. 0

3. 1.5

4. 1

When the initial concentration of the reactant is doubled, the half-life period of a zero-order reaction is:

1.	Halved	2.	Doubled
3.	Tripled	4.	Unchanged

The half-life for a zero-order reaction having 0.02 M initial concentration of reactant is 100 s. The rate constant (in mol L^–1 s^–1) for the reaction is:

1. $1.0\backslash times{10}^{-4}$

2. $2.0\backslash times{10}^{-4}$

3. $2.0\backslash times{10}^{-3}$

4. $1.0\backslash times{10}^{-2}$

The given graph is a representation of the kinetics of a reaction.

The y and x axes for zero and first-order reactions, respectively are:

1.	zero order (y=rate and x=concentration), first order (y=rate and x=t1/2)
2.	zero order (y=concentration and x=time), first order (y=t1/2 and x = concentration)
3.	zero order (y=concentration and x= time), first order (y=rate constant and x= concentration)
4.	zero order (y=rate and x=concentration), first order (y=t1/2 and x = concentration)

For a certain reaction, the rate = when the initial concentration of A is tripled keeping the concentration of B constant, the initial rate would be:

1.	Increase by a factor of three
2.	Decrease by a factor of nine
3.	Increase by a factor of six
4.	Increase by a factor of nine