Question

A transition state represents the state of highest energy in passing from reactant to product. If true enter 1, if false enter 0

Answer 1

To answer this question, you should recall the concept of transition state as well as the concept of collision theory and activation energy. During a reaction, the reactants possessing required activation energy are first converted to unstable transition state compounds and then to products.

Complete step by step answer:
According to the collision theory, as the molecules of reactant entities are assumed to be hard spheres and the reactions are assumed to occur only when these spheres collide with each other”. So the term collision frequency was developed to quantify the number of collisions occurring in order to form products so that we can have a clear picture of the reaction.
Transition-state theory, also called activated-complex theory or theory of absolute reaction rates, treatment of chemical reactions and other processes that regards them as proceeding by a continuous change in the relative positions and potential energies of the constituent atoms and molecules.
On the reaction path between the initial and final arrangements of atoms or molecules, there exists an intermediate configuration at which the potential energy has a maximum value. The configuration corresponding to this maximum is known as the activated complex, and its state is referred to as the transition state.

Hence, the given statement is correct and the final answer is 1.

Note:
Collision Frequency can be understood as the number of collisions per second per unit volume of the reacting mixture. It is generally denoted by $Z$. One more parameter that affected the rates of chemical reactions significantly is activation energy. The term activation energy was given by Arrhenius, it is the minimum amount of energy that the reactants must possess in order to form a product during a chemical reaction.