C8 - Rates and equilibrium 2️⃣✅

A point where both reactions are taking place at the same time so it looks like there is no change/ are happening at the exact same rate and will follow La Chatelier’s principle to change/ move to reistablish equilibrium

That a sysytem will do the opposite in order to reistablish equilibrium

The measure of the speed at which something happens in a given time

• Presence of a catalyst • Temperature • Concentration & pressure • Surface area of solids

Catalysts work by providing alternate reaction pathways to the products with a lower activiation energy than without the catalysts present to increase the rate of reaction

By heating up a substance more kinetic energy is generated and therefore particles move around faster and therefore collide much more frequently. When particles collide more frequently there is an increased chance they will react, therefore increasing the rate of reaction

By increasing the pressure, there is less space avainable for particles to move therefore increasing the frequency of collisions and therefore increases rate of reaction. Increasing the concentration of reactants causes more frequent collisions and therefore increases rate of reaction.

Only reactant particles are capable of colliding and reacting, therefore by increasing the surface area you are increasing the number of reactant particles exposed, leading to more frequent collisions and therefore increasing rate of reaction

The idea that in order for a reaction to occur paricles must collide, and that in order for particles to react when they collide they must surpass the activation energy - minimunm ammount of energy for a collision to be sucsesful/ to collide and therefore react

it will be endothermic in the other

When a reactions reactants can turn into products and the products can turn into the reactants

That something contains water

That something does not contain water

If the concentration of a reactant is increased, more products will be formed until equilibrium is reached again.

If the concentration of a product is decreased, less reactants will react until equilibrium is reached again.

• Endothermic reaction direction is favoured • The ammount of products increases for an endothermic reaction • The ammount of products decreases for an exothermic reaction

• Exothermic reaction direction is favoured • The ammount of products decreases for an endothermic reaction • The ammoun of products increases for an exothermic reaction

• Favour direction/side with the fewest number of molocules • An increase in pressure causes the equilibrium position to shift towards (favour) the side with the smaller number of molecules as shown by the symbol equation for that reaction

• Favour direction/side with the largest number of molocules • An decrease in pressure causes the equilibrium position to shift towards (favour) the side with the larger number of molecules as shown by the symbol equation for that reaction

When, in a reversible reaction the forward and reverse reactions occur at exactly the same rate/ are taking place at the same time so it looks like there is no change/ are happening at the exact same rate

The minimum ammount of energy that particles must have to react

the quality of a substance/ solvent being cloudy/ opaque

• Measuring loss of mass • Volume of gass produced • Colour Change • Turbidity of a reaction mixture