Temperature dependence of reaction rates

The activation energy for the reaction $2\mathrm{HI}\left(\mathrm{g}\right)\to {\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)$  is $209.5{\mathrm{kJmol}}^{-1}$ at $581\mathrm{K}$. The fraction of molecules having energy equal to or greater than activation energy is: $[\mathrm{R}=8.31{\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}]$

Activation energy can be calculated by using the relation,

$\ln \frac{{\mathrm{k}}_2}{{\mathrm{k}}_1}=-\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{R}}\left[\frac{1}{{\mathrm{T}}_1}-\frac{1}{{\mathrm{T}}_2}\right]$

The rate constant of a reaction at temperature $200 \mathrm{K}$ is $10$ times less than the rate constant at $400 \mathrm{K}.$ What is the activation energy $\left({\mathrm{E}}_{\mathrm{a}}\right)$ of the reaction$?$

The rate constant of a reaction at temperature $200 \mathrm{K}$ is $10$ times less than the rate constant at $400 \mathrm{K}.$ What is the activation energy $\left({\mathrm{E}}_{\mathrm{a}}\right)$ of the reaction$?$

($\mathrm{R}=$ Gas constant)

How to calculate activation energy if the value of rate constant given at two different temperatures.

Discuss the concept of energy distribution in molecules and also give the graphical representation of fraction of molecules versus kinetic energy.

In the Arrhenius equation, the universal gas constant can be replaced by

Define Arrhenius concept of chemical kinetics.

Among the following graphs showing variation of rate constant with temperature ($\mathrm{T}$) for a reaction, the one that exhibits Arrhenius behaviour over the entire temperature range is

The rate constant of the first-order reaction, i.e., decomposition of ethylene oxide into ${\mathrm{CH}}_4$ and $\mathrm{CO}$ may be described by the following equation: $\log \mathrm{k} \left({\mathrm{s}}^{-1}\right)=14.34-\frac{1.25\times {10}^4}{\mathrm{T}}\mathrm{K}.$

Find the energy of activation (in kJ/mole). Report answer till the nearest integer.

In the $\ln \mathrm{K }v\mathrm{s }\frac{1}{T}$ plot of a chemical process having $∆S^0>0$ and $∆H^o<0$ the slope is proportional to (where $K$ is equilibrium constant)

For a first order chemical reaction, 

Which among the following equations represents Arrhenius equation ?

For a first order reaction, $\mathrm{A}\to \mathrm{B}, \mathrm{logk} \mathrm{vs} 1/\mathrm{T}$ the curve has a gradient of $-5000 \mathrm{K}$. The activation energy of the reaction in $\mathrm{kJ}/\mathrm{mol}$ is ______
($\mathrm{R}$ is the ideal gas constant).

The Arrhenius equation is

The rate constant of a reaction

A first order gas-phase reaction has an energy of activation of $240 \mathrm{kJ} {\mathrm{mol}}^{-1}$. If the frequency factor of the reaction is $1.6 \mathrm{x} {10}^{13}$, calculate its rate constant at $600 \mathrm{K}$
 

The rate constant of a first order reaction at $25° \mathrm{C}$ is $0.24 {\mathrm{s}}^{-1}$. If the energy of activation of the reaction is $88 \mathrm{kJ} {\mathrm{mol}}^{-1}$, at what temperature would this reaction have rate constant of $4 \mathrm{x} {10}^{-2} {\mathrm{s}}^{-1}?$