Temperature Dependence of the Rate of a Reaction

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: $[\mathrm{R}=8.31{\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}]$

The factors which influence the rate of reaction are :

Concentration: Greater the concentrations of the reactants, faster is the rate of reaction.

Temperature: The rate of reaction increases with increase in temperature. For most of the reactions, the rate of reaction becomes almost double with 10o rise in temperature.

Presence of catalyst: A catalyst generally increases the speed of a reaction.

Answer the following question :

The role of a catalyst is to change _____.

The factors which influence the rate of reaction are :

Concentration: Greater the concentrations of the reactants, faster is the rate of reaction.

Temperature: The rate of reaction increases with increase in temperature. For most of the reactions, the rate of reaction becomes almost double with 10o rise in temperature.

Presence of catalyst: A catalyst generally increases the speed of a reaction.

Answer the following question :

A small increase in temperature of the reacting system, the rate of reaction exceed to large extend. The most appropriate reason for this is-

What is an inhibitor and what does it do?

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

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)

After rise in temperature, the activation energy will:

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).

What type of inhibitor is aspirin?

Penicillin acts as an inhibitor.

The activation energy for a reaction at the temperature $\mathrm{T} \mathrm{K}$ was found to be $2.303\mathrm{RT} \mathrm{J} {\mathrm{mol}}^{-1}$. The ratio of the rate constant to Arrhenius factor is

If the activation energy for the forward reaction is $150 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and that of the reverse reaction is $260 \mathrm{kJ} {\mathrm{mol}}^{-1}$, what is the enthalpy change for the reaction?

If a reaction $\mathrm{A}+\mathrm{B}\to \mathrm{C}$ is exothermic to the extent of $30 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and the forward reaction has an activation energy $70 \mathrm{kJ} {\mathrm{mol}}^{-1}$, the activation energy for the reverse reaction is