Arrhenius Collision Theory

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

For the adsorption of hydrogen on platinum, the activation energy is $30 \mathrm{kJ} {\mathrm{mol}}^{–1}$ and for the adsorption of hydrogen on nickel, the activation energy is $41.4 \mathrm{kJ} {\mathrm{mol}}^{–1}.$ The logarithm of the ratio of the rates of chemisorption on equal areas of the metals at $300 \mathrm{K}$ is $\_\_\_\_\_\_\_$ (Nearest integer)

Given: $\mathrm{In}10=2.3$

$\mathrm{R}=8.3 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$

The correct reaction profile diagram for a positive catalyst reaction.

For the reaction ${\mathrm{CO}}_{\left(\mathrm{g}\right)}+{\mathrm{Cl}}_{2\left(\mathrm{g}\right)}\to {\mathrm{COCl}}_{2\left(\mathrm{g}\right)}$ under the same concentration conditions of the reactants, the rate of reaction at ${250}^{\mathrm{o}}\mathrm{C}$ IS 1500 times as fast as the same reaction at ${150}^{\mathrm{o}}\mathrm{C}$. Calculate the activation energy of the reaction.If the frequency factor is $2 \times {10}^{-10}$${\mathrm{M}}^{-1}{\sec }^{-1}$ Calculate the rate constant of the reaction at ${150}^{\mathrm{o}}\mathrm{C}$.

A bottle of milk stored at $300 \mathrm{K}$ sours in $36 \mathrm{hours}$. When stored in a refrigerator at $275 \mathrm{K}$ it sours in $360 \mathrm{hours}.$ Calculate the energy of activation $\left(\text{in} \mathrm{kJ}/\mathrm{mole}\right)$ of the reaction involved in the souring process. $\left(\mathrm{R}=8.314 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}\right)$.

Give the nearest integer as the answer.

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.

A certain physiologically important first-order reaction has activation energy equal to $45.0 \mathrm{kJ} {\mathrm{mol}}^{-1}$ at normal body temperature $\left(37 °\mathrm{C}\right).$Without a catalyst, the rate constant for the reaction is $5.0\times {10}^{-4}{\mathrm{s}}^{-1}$. To be effective in the human body, where the reaction is catalysed by an enzyme, the rate constant must be at least $2·0\times {10}^{-2}{\mathrm{s}}^{-1}.$ If the activation energy is the only factor affected by the presence of the enzyme, by how much must the enzyme lower the activation energy of the reaction to achieve the desired rate? (Report your answer by multiplying with 10 and rounding off to two significant figures)

A certain physiologically important first-order reaction has an activation energy equal to $45.0 \mathrm{kJ}/\mathrm{mol}$ at normal body temperature $\left(37°\mathrm{C}\right).$ Without a catalyst, the rate constant for the reaction is $5.0\times {10}^{-4} {\mathrm{s}}^{-1}$. To be effective in the human body, where the reaction is catalysed by an enzyme, the rate constant must be at least  $2.0\times {10}^{-2} {\mathrm{s}}^{-1}$. If the activation energy is the only factor affected by the presence of the enzyme, by how much $\mathrm{kJ}$ must the enzyme lower the activation energy of the reaction to achieve the desired rate?

Report the answer by multiplying the value with 10 and rounding off to two significant figures.

A certain physiologically important first-order reaction has activation energy equal to $45.0 \mathrm{kJ} {\mathrm{mol}}^{-1}$at a normal body temperature $\left(37 °\mathrm{C}\right).$ Without a catalyst, the rate constant for the reaction is $5·0\times {10}^{-4}{\mathrm{s}}^{-1}$. To be effective in the human body, where the reaction is catalysed by an enzyme, the rate constant must be at least $2·0\times {10}^{-2}{\mathrm{s}}^{-1}$. If the activation energy is the only factor affected by the presence of the enzyme, by how much must the enzyme lower the activation energy of the reaction to achieve the desired rate? Give answer to the nearest integer  value after multiplying with 10.

A hydrogenation reaction is carried out at $500 \mathrm{K}.$ If the same reaction is carried out in the presence of a catalyst at same rate, the temperature required is $400 \mathrm{K}$ and if the catalyst lowers the activation energy by $20 \mathrm{kJ} {\mathrm{mol}}^{-1}$, the activation energy of uncatalyzed reaction at $500 \mathrm{K}$ will be:

The rate of a reaction decreased by $3.555$ times when the temperature was changed from $40°\mathrm{C}$ to $30°\mathrm{C}$. The activation energy (in ${\mathrm{KJmol}}^{-1}$) of the reaction is.........(Report the answer in the nearest integer value)

[Take; $\mathrm{R}=8.314 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$ and  $\ln$ $3.555=1.268$]

For the reaction, $\mathrm{aA}+\mathrm{bB}\to \mathrm{cC}+\mathrm{dD}$, the plot of $\log \mathrm{k}$ vs $\frac{1}{ \mathrm{T}}$ is given below:

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)

Which among the following equations represents Arrhenius equation ?

The rate constant of a reaction is given by $\mathrm{k}={\mathrm{PZe}}^{-\mathrm{Ea}/\mathrm{RT}}$ under standard notation In order to speed up the reaction, which of the following factors has to he decreased?

The activation energy for the forward reaction, $\mathrm{P}\to \mathrm{Q}$ is $20 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and the enthalpy change, $\mathrm{\Delta H}$ of the reaction is $+10 \mathrm{kJ} {\mathrm{mol}}^{-1}$. The activation energy (in $\mathrm{kJ} {\mathrm{mol}}^{-1}$) for the backward reaction will be

Raw milk sours in $4$ hours at $27°\mathrm{C}$, but in $40$ hours in refrigerator at $7°\mathrm{C}$. What is activation energy (in $\mathrm{KJ}$). for souring milk.

[Given $\mathrm{R}=8.3 \mathrm{J}/\mathrm{mole}-\mathrm{k}, \ln x=2.3 \mathrm{logx}]$

Round off your answer to the nearest integer.