Collision Theory of Chemical Reaction

At a temperature of $\mathrm{T}=300 \mathrm{K}$ there are $30\%$ molecules with kinetic energy greater than the activation energy. According to Arrhenius equation, the fraction of the molecules which will have kinetic energy greater than the activation energy at $150 \mathrm{K}$ [Assume that the activation energy is independent of temperature] is

In a reversible reaction, the enthalpy change and the activation energy in the forward direction are respectively $-\mathrm{x} \mathrm{kJ} {\mathrm{mol}}^{-1}$ and $\mathrm{y} \mathrm{kJ} {\mathrm{mol}}^{-1}$. Therefore, the energy of activation in the backward direction is

Collision theory is applicable to 

Collision theory is satisfactory for:-

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

What is the activation energy of the reaction B→A, if ${\mathrm{E}}_{\mathrm{a}}$ for the reaction $\mathrm{A}\to \mathrm{B}$ is 120 kJ/mole of A. The enthalpy of reaction is –140 kJ/mole.

In the potential energy profile, the intermediate species corresponding to point$3$, is

The pre-exponential factor for free radical addition of chlorine is ${\text{2 × 10}}^{13} s^{–1}$. Figure out the rate constant of this reaction at $\mathrm{STP}$, given $\mathrm{R} = 8.314 \mathrm{J} {\mathrm{mol}}^{–1} {\mathrm{K}}^{–1}$ ?

Which is correct according to the collision theory of chemical reactions?

Increase in concentration of the reactants can lead to change in:

Statement - 1: If number of gaseous molecules per unit volume are doubled, collision frequency becomes four times of initial. and

Statement - 2:

Collision frequency $n= \sqrt{2} \pi {\sigma }^2{N}^{2}v$ .

For the equilibrium, $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right),\mathrm{ }∆\mathrm{H}-40\mathrm{ }$ kJ/mol. If the ratio of the activation energies of the forward $\left({\mathrm{E}}_{\mathrm{f}}\right)$ and revers $\left({\mathrm{E}}_{\mathrm{b}}\right)$ reactions is $\frac{2}{3}$ then:

The molecular diameter of $\mathrm{A}$ and  $\mathrm{B}$ are $4\mathrm{ }\mathrm{n}\mathrm{m}$ and $8\mathrm{ }\mathrm{n}\mathrm{m}$ respectively. The pressure of $\mathrm{A}$ and $\mathrm{B}$ are 10 atm and 5 atm respectively. The temperature of $\mathrm{A}$ and $\mathrm{B}$ are $300\mathrm{ }\mathrm{K}$ and $400\mathrm{ }\mathrm{K}$ respectively. The ratio of molecular mass of $\mathrm{A}$ and $\mathrm{B}$ are $30\mathrm{ }:\mathrm{ }40$. What will be the ratio of binary collisions among $\mathrm{A}$ molecules to that of $\mathrm{B}$ molecules ?

Increase in the concentration of the reactants leads to the change in

What istThe minimum energy required for a molecule to take part in a reaction is called?

Collision theory is applicable to which of the following?

Collision theory is applicable to which of the following?

Which of the following statements is under collision theory?

$\left(\mathrm{I}\right)$ Rate is directly proportional to collision frequency.

$\left(\mathrm{II}\right)$ The rate depends upon the orientation of atoms.

$\left(\mathrm{III}\right)$ Temperature determines the rate.

A chemical reaction proceeds the following formula:

$\mathrm{k}={\mathrm{PZe}}^{-{\mathrm{E}}_{\mathrm{a}}/\mathrm{RT}}$

Which of the following processes will increase the rate of reaction?

The rate of reaction increases with temperature due to