Rate of a general reaction A+B arrow products can be expressed as follows on the basis of collision theory. Rate=ZABe-Ea /RT Which of the following statements is not correct for the above expression?

Question

Rate of a general reaction A+B arrow products can be expressed as follows on the basis of collision theory. Rate=ZABe-Ea /RT Which of the following statements is not correct for the above expression? (A) Z is collision frequency and is equal to number of collisions per second per unit volume of the reaction mixture. (B) e-Ea /RT is the fraction of molecules with kinetic energy equal to or greater than Ea. (C) Ea is activation energy of the reaction. (D) All the molecules which collide with one other are effective collisions.

Tardigrade Admin · Accepted Answer

Only those collisions in which molecules collide with sufficient energy, called threshold energy and proper orientation are effective collisions. Rest of the molecules collide and bounce back.

Q. Rate of a general reaction $A + B$ $\to$ products can be expressed as follows on the basis of collision theory. Rate= $Z_{A B^{e^{- E_{a} / RT}}}$ Which of the following statements is not correct for the above expression?

$Z$ is collision frequency and is equal to number of collisions per second per unit volume of the reaction mixture.

$e^{- E_{a} / RT}$ is the fraction of molecules with kinetic energy equal to or greater than $E_{a} .$

$E_{a}$ is activation energy of the reaction.

All the molecules which collide with one other are effective collisions.

Only those collisions in which molecules collide with sufficient energy, called threshold energy and proper orientation are effective collisions. Rest of the molecules collide and bounce back.

Q. Rate of a general reaction A+B → products can be expressed as follows on the basis of collision theory. Rate=ZABe−Ea​/RT​ Which of the following statements is not correct for the above expression?

Z is collision frequency and is equal to number of collisions per second per unit volume of the reaction mixture.

e−Ea​/RT is the fraction of molecules with kinetic energy equal to or greater than Ea​.

Ea​ is activation energy of the reaction.

All the molecules which collide with one other are effective collisions.

Only those collisions in which molecules collide with sufficient energy, called threshold energy and proper orientation are effective collisions. Rest of the molecules collide and bounce back.

Q. Rate of a general reaction $A + B$ $\to$ products can be expressed as follows on the basis of collision theory. Rate= $Z_{A B^{e^{- E_{a} / RT}}}$ Which of the following statements is not correct for the above expression?

$Z$ is collision frequency and is equal to number of collisions per second per unit volume of the reaction mixture.

$e^{- E_{a} / RT}$ is the fraction of molecules with kinetic energy equal to or greater than $E_{a} .$

$E_{a}$ is activation energy of the reaction.