Answer: A. enough kinetic energy and favorable geometry
Explanation: According to collision theory, the rate of a reaction depends upon the number of effective collisions which means the collisions which result in the formation of product which in turn depend on following two factors:-
a) Energy factor: In order for a collision to be successful, the colliding molecules must cross a energy barrier which is called as threshold energy. Thus molecules with energy less than threshold energy are not able to result into products.
b) Orientation factor: the colliding molecules must have proper orientations at the time of collision otherwise they do not result in product formation.
The correct option is this: EFFUSION BECAUSE THERE IS A MOVEMENT OF A GAS THROUGH A SMALL OPENING INTO A LARGER VOLUME. Effusion refers to the movement of gas particles through a small hole. According to Graham's law, the effusion rate of a gas is inversely proportional to the square root of the mass of its particles.
C: It depends on the entropy and enthalpy of the reaction.
Explanation:
Gibbs free energy is defined as the maximum amount of non-expansion work that can be gotten from a closed system. Now this work is usually done in place of the system’s internal energy and Energy that is not extracted as work is usually exchanged with the immediate surroundings in the form of heat.
