A reaction proceeds via a two-step mechanism. The first step is a fast, reversible equilibrium with a small equilibrium constant. The second step is slow. Which of the following is MOST likely true about the overall reaction rate?

Which factor has the LEAST impact on the rate of a reaction involving large, complex biomolecules?

The threshold energy of a chemical reaction depends upon:

The rate of a specific chemical reaction is significantly increased by the introduction of a catalyst. Which of these factors associated with the reaction remains unaltered?

If $X$ is the total number of collisions which a gas molecule register with others per unit time under particular conditions, then the collision frequency of the gas containing $N$ molecules per unit volume is

Which of the following statement is in accordance with collision theory?

I. Rate is directly proportional to collision frequency

II. Rate depend upon orientation of atoms

III. temperature determines the rate

The pre-exponential factor (A) in the Arrhenius equation is related to the:

For a reaction to occur according to collision theory, the colliding molecules must have:

In a reaction, the threshold energy is equal to:

An increase in the concentration of reactants of a reaction leads to change in

The activation energies of forward and backward reaction: ${A_2} + {B_2}\leftrightharpoons2AB$ are 180kJ ${\rm{mo}}{{\rm{l}}^{ - 1}}$ and 200 kJ ${\rm{mo}}{{\rm{l}}^{ - 1}}$ respectively. The presence of a catalyst lowers the activation energy of both (forward and backward) reactions by 100 kJ ${\rm{mo}}{{\rm{l}}^{ - 1}}$. The enthalpy change of the reaction in the presence of catalyst will be (in kJ ${\rm{mo}}{{\rm{l}}^{ - 1}}$):