Chapter 10 - Reaction rates and Equilibrium Flashcards
rate of reaction
➜ measures how fast a reacant is being used up or how fast a product is being formed
Factors effecting ROR
➜ concentration - increased number of particles in same volume = particles collide more frequently
➜ pressure - more particles in a smaller volume = more collisions
➜ temperature - more kinetic energy to overcome energy barrier = particle speed increases for more collisions
➜ catalyst - alternate pathway with lower Eₐ = particles have sufficient energy to overcome Eₐ now that its low
➜ surface area of solid reactants - increased chance of collision = more particles exposed
Collision theory
➜ states that 2 reacting particles must collide for a reaction to occur
↳ must collide with correct orientation
↳ particles have sufficient energy to overcome the Eₐ barrier of reaction
Eₐ
minimum energy required to start a reaction by the breaking of bonds
Boltzmann curve
➜ no molecules have 0 energy -= curve starts at origin
➜ area under the curve = number of molecules
➜ area before Eₐ = unsuccessful particles that didn’t react due to lack of energy
➜ area after Eₐ = successful particles that reacted
Le Chatlier’s principle
➜ states that when a system in equilibrium is subjected to an external change the system readjusts itself to minimise the effect of that change
Dynamic equilibrium
➜ the equilibrium that exists in a closed system when the rate of the forward reaction is equal to the reverse reaction and concs do not change
Effect of CONC on equilibrium
➜ If there are more products being formed equilibrium is shifted to the right and vice versa
Effect of TEMP on equilibrium
➜ Increase in temp favours the endothermic side (+)
➜ decrease in temp favours exothermic side (-)
Effect of PRESS on equilibrium
➜ increasing pressure shifts equilibrium to the side with LESS moles of gas
➜ decreasing pressure shifts equilibrium to the side with MORE moles of gas
Kc
products to the power of their co efficient OVER reactants to the power of their co efficient
