IQ2 Flashcards
decreasing pressure of system
shifts equilibrium towards side with more gaseous moles
increasing pressure of system
shifts equilibrium towards side with fewer gaseous moles
increase the concentration of a product
shifts equilibrium to the reactants
increase the concentration of a reactant
shifts equilibrium to the products
what is Le Chatelier’s principle
When a system in equilibrium is subjected to a change in concentration, temperature, external pressure, or some other factor which upsets the equilibrium, the system reacts in such a way as to counteract that change.
increasing temperature of the system
favour endothermic reaction to absorb extra heat energy
decrease temperature of the system
favour the exothermic reaction to produce extra heat energy
positive delta H goes
reactants
negative delta H goes
products
what does increasing temperature do (Collison theory)
Increasing heat energy increases kinetic energy of the particles. This increases their velocity. This also means they are more likely to have sufficient energy to overcome the activation energy needed for the reaction to occur. This increases the frequency of collisions and improves the chances of successful reactions when a collision occurs.
what does increasing concentration do (Collision theory)
Increasing the concentration of a substance increases the numbers of particles and hence there is a higher likelihood of reactant particles colliding to form one or more products, or vice versa
what does increasing pressure do (Collision theory)
Increasing pressure for gases involves increasing the density or decreasing the volume. Pushing the same number of particles into a smaller space will increase the likelihood of collisions hence increase the rate of reaction.
