Kinetics

the time it takes for all the reactants to have been used up/all the products to have been formed

change/time

temperature concentration light catalysts pressure in gasesous reactants surface area in solid reactants

at the beginning of the reaction due to the higher concentration of reactants

According to the collision theory, reactions can only occur when: • Reactants collide in the correct orientation. • Reactants have the enough energy to form its products. • activation and suficent kinetic energy is required

the minimum energy needed for a reaction to occur

• range of energy/Users/mayrasalazar/Downloads/51c06e6ee4b0a49e8c8f47e6-aaronq-1371569791668-screen_shot_20120502_at_11212_pm1335978747666-2.png

temperature

a collision which results in a reaction, more succesful collions= increase of rate in a reaction

increase the rate as there is a higher number of successful collisions

• decrease particle size, as only surface molecules react

increase concentration ideal gas concentration

increases the kinetic energy, increases the rate of reaction, increases fruitful collisions - shifts distribution graph

a substance that increases the rate without reacting itself

A chemical reaction is essentially involves two processes, bond breaking and bond forming. As mentioned in the Energetics chapter, particles tend to react to become more stable.

Collision theory – reactions take place as a result of particles (atoms or molecules) colliding and then undergoing a reaction. Not all collisions cause reaction, however, even in a system where the reaction is spontaneous. The particles must have sufficient kinetic energy, and the correct orientation with respect to each other for the two to react. Even then, the transition state may revert to the reactant molecules instead of forming the product molecules.

the study of the factors that affect the ROR