EXERCISE-2

At certain temperature, the half life period in the thermal decomposition of a gaseous substance as follows:

Find the order of reaction [Given $\log (23.5)=1.37;\log \left(95\right)=1.97]$

A first order reaction is $25\%$ completed in $20$ minutes at $300 \mathrm{K}$. When same reaction in carried out at $320 \mathrm{K}$, it is $25\%$ complete in 5 minute. What is the activation energy of reaction (in $\mathrm{kJ}/\mathrm{mole}$ )?

[Take : $\mathrm{R}=8 \mathrm{J}/\mathrm{K}$ mole and $\ln 2=0.7]$

 Consider the reaction

   .

The rate constant for two parallel reactions were found to be ${10}^{-2}{\mathrm{dm}}^3{ \mathrm{mol}}^{-1}{ \mathrm{s}}^{-1}\left({\mathrm{k}}_1\right)$ and $4\times {10}^{-2}{\mathrm{dm}}^2{ \mathrm{mol}}^{-1}{ \mathrm{s}}^{-1}\left({\mathrm{k}}_2\right)$ 

If the corresponding energies of activation of the parallel reactions are $80$ and $100 \mathrm{kJ}$  respectively. What is the apparent (net) overall energy of activation of given reaction.

For the reaction $\mathrm{A}\to \mathrm{B}$, the rate law expression is $-\frac{\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}=\mathrm{k}{\left[\mathrm{A}\right]}^{1/2}$. If initial concentration of $\left[\mathrm{A}\right]$ is ${\left[\mathrm{A}\right]}_0$, then :

For the first order decomposition of ${\mathrm{SO}}_2{\mathrm{Cl}}_2\left(\mathrm{g}\right)$,

$\left[{\mathrm{SO}}_2{\mathrm{Cl}}_2\left(\mathrm{g}\right)\to {\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)\right]$

a graph of $\log \left({\mathrm{a}}_0-\mathrm{x}\right)$ vs $\mathrm{t}$ is shown in figure. What is the rate constant $\left({\sec }^{-1}\right)$ ?

Consider the reaction $\mathrm{A}⟶\mathrm{B}$, graph between half life $\left({\mathrm{t}}_{1/2}\right)$ and initial concentration (a) of the reactant is

Hence, graph between$-\frac{\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}$ And time will be

Select incorrect statement (s):

$\mathrm{A}\to \mathrm{B}$      ${\mathrm{K}}_{\mathrm{A}}={10}^{15}{\mathrm{e}}^{-2000/\mathrm{T}}$

$\mathrm{C}\to \mathrm{D}$     ${\mathrm{K}}_{\mathrm{C}}={10}^{14}{\mathrm{e}}^{-1000/\mathrm{T}}$

Temperature $\mathrm{TK}$ at which $\left({\mathrm{K}}_{\mathrm{A}}={\mathrm{K}}_{\mathrm{C}}\right)$ is :