Chemistry Chemical Kinetics

The reaction rate for the reaction

${\left[PtC{l}_4\right]}^{2-}+H_{2}O\stackrel{}{?}{\left[Pt\left(H_{2}O\right)C{l}_3\right]}^{-}+C{l}^{-}$            

was measured as a function of concentrations of different species. It was observed that  

$\frac{-d{\left[\left[PtC{l}_4\right]\right]}^{2-}}{dt}=4.8*10^{-5}\left[{\left[PtC{l}_4\right]}^{2-}\right]-2.4*10^{-3}\left[{\left[Pt\left(H_{2}O\right)C{l}_3\right]}^{-}\right]\left[C{l}^{-}\right]$

where square bracket are used to denote molar concentrations. The equilibrium constant K_C = ________. (Nearest integer)

Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R).

Assertion (A): Heavy water is used for the study of reaction mechanism.

Reason (R): The rate of reaction for the cleavage of O-H bond is slower than that of O-D bond.

Choose the most appropriate answer from the options given below:

At 345 K, the half life for the decomposition of a sample of a gaseous compound initially at 55.5 kPa was 340s. When the pressure was 27.8 kPa., the half life was found to be 170s. The order of the reaction is ________. [integer answer]

2NO + 2H₂ ® N₂ + 2H₂O

The above reaction has been studied at 800°C. The related data are given in the table below.

The order to the reaction with respect to NO is_______________.

The rate constant for a first order reaction is given by the following equation Ink = 33.24 - $\frac{2.0*10^{4}K}{T}$  

The activation energy for the reaction is given by ___________kJ mol^-1 (In nearest integer) (Given: R = 8.3JK^-1mol^-1)

For the reaction

$2{\mathrm{H}}_2\left(\mathrm{g}\right)+2\mathrm{N}\mathrm{O}\left(\mathrm{g}\right)?{\mathrm{N}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}$ , the observed rate expression is, rate = ${\mathrm{k}}_{\mathrm{f}}[\mathrm{N}\mathrm{O}{]}^2\left[{\mathrm{H}}_2\right]$ . The rate expression for the reverse reaction is:

[A]               ->                     [B]

Reactant                         Product

If formation of compound [B] follows the first order of kinetics and after 70 minutes the concentration of [A] was found to be half of its initial concentration. Then the rate constant of the reaction is x * 10^-6 s^-1. The value of x is___________. (Nearest Integer)

2NO + 2H₂ → N₂ + 2H₂O

The above reaction has been studied at 800°C. The related data are given in the table below.

The order to the reaction with respect to NO is_______________.

For the decomposition of azomethane,

CH₃N₂CH₃(g) → CH₃CH₃(g) + N₂(g), a first order reaction, the variation in partial pressure with time at 600 K is given as.

The half life of the reaction is __________* 10^-5s. [Nearest integer]