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

From the following data ${\mathrm{H}}_{2 }+ {\mathrm{I}}_2 \to 2\mathrm{HI}$

Which of the following is the appropriate ${\mathrm{E}}_{\mathrm{a}}$ of the reaction?

The plot of ${\mathrm{logk}}_{\mathrm{f}}$ versus $\frac{1}{\mathrm{T}}$ for a reversible reaction $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{P}\left(\mathrm{g}\right)$ is shown.

Pre-exponential factors for the forward and backward reactions are ${10}^{15} {\mathrm{s}}^{-1}$ and ${10}^{11} {\mathrm{s}}^{-1}$, respectively. If the value of $\mathrm{logK}$ for the reaction at $500 \mathrm{K}$ is $6$, the value of $\left|{\mathrm{logk}}_{\mathrm{b}}\right|$ at $250 \mathrm{K}$ is
$\left[\mathrm{K}=\right.$equilibrium constant of the reaction, ${\mathrm{k}}_{\mathrm{f}}=$rate constant of forward reaction, ${\mathrm{K}}_{\mathrm{b}}=$rate constant of backward reaction]

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

Assertion A: A reaction can have zero activation energy

Reason R: The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value, is called activation energy.

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 number of given statement/s which is/are correct is_____

(A) The stronger the temperature dependence of the rate constant, the higher is the activation energy.

(B) If a reaction has zero activation energy, its rate is independent of temperature.

(C) The stronger the temperature dependence of the rate constant, the smaller is the activation energy.

(D) If there is no correlation between the temperature and the rate constant then it means that the reaction has negative activation energy.

Consider the following reaction that goes from $\mathrm{A}$ to $\mathrm{B}$ in three steps as shown below:

Choose the correct option

The rate constant for the reaction: ${\mathrm{CH}}_3\mathrm{CHO}\left(\mathrm{g}\right) \to {\mathrm{CH}}_4\left(\mathrm{g}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$ are $0.035 {\mathrm{M}}^2{\mathrm{S}}^{-1} \mathrm{at} 730\mathrm{K} \mathrm{and} 0.343 {\mathrm{M}}^2 \mathrm{at} 790\mathrm{K}$

Calculate activation energy of the reaction.($\mathrm{R}=8.314{\mathrm{Jk}}^{-1}{\mathrm{mol}}^{-1}$)

The rate constants of a reaction at $400 \mathrm{K} \mathrm{and} 600 \mathrm{K}$ are $5 \mathrm{x} {10}^{-3} \mathrm{s}{ }^{–1} \mathrm{and} 8 \mathrm{x} {10}^{-3} \mathrm{s}{ }^{–1}$ respectively. What extra piece of information is needed to calculate the value of $\mathrm{A}$ (frequency factor)?

(According to the Arrhenius equation, rate constant is given by, $\mathrm{k} = {\mathrm{Ae}}^{-\mathrm{E}{ }_{\mathrm{a} }/\mathrm{RT}}.$)

Kamlesh was conducting an experiment to figure out the rate equation of the following reaction:

$2 \mathrm{NO} + {\mathrm{O}}_2 --> 2 {\mathrm{NO}}_2$

He measured the rate of this reaction as a function of initial concentrations of the reactants as follows:

Which of the following could be a reason for the inconsistency in the initial rate of formation of ${\mathrm{NO}}_2$ data for experiment $4$?

Draw the graphical representation of arrenhious equation.

If rate of reaction increases by a factor of 2, when temperature is raised from $27°\mathrm{C} \mathrm{to} 37°\mathrm{C}$. What is the value of activation energy in kJ/mol? By what factor does rate of reaction increase if temperature is increased from $127°\mathrm{C} \mathrm{to} 137°\mathrm{C}.$
$[\mathrm{Given}: \ln 2=0.7, \mathrm{R}= 8.314 \mathrm{Joule}/\mathrm{mol}.\mathrm{K}, {\mathrm{e}}^{0.4}=1.5]$
(a) If temperature coefficient is same in given temperature range
(b) If temperature coefficient is function of temperature.

If the definition of the temperature coefficient of the reaction holds good for a reaction between $27°\mathrm{C}$ and $37°\mathrm{C}$, the activation energy for the reaction in $\mathrm{kJ}.{\mathrm{mol}}^{-1}$ is

The rate constant of a reaction is increased $4$ times after addition of catalyst to the reaction mixture at the same temperature of $27 °\mathrm{C}$. The change in the activation energy of this reaction is
(Take $\ln \left(\frac{1}{4}\right)=-1.386,\mathrm{R}=8.314$)

The potential energy diagram for four reactions are given below

Which one of the following statements about these diagrams is incorrect?

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 ${150}^{\mathrm{o}}\mathrm{C}$.