C6

• a reversible reaction is a reaction that can go from reactants to products and form products to reactants
• a reaction is at equilibrium when some product is removed, so the forwards reaction will increase as that will increase the amount of product
• a catalyst is something that changes the rate of reaction but it not used up in the reaction
• by increasing the pressure, this affects equilibrium because it favours the side with fewer gaseous particles
• the unit to measure the rate of reaction when measuring how quickly a gas is produced is: cm3/s
• the effect of increasing the pressure of a gas on the rate of reaction is that the rate of reaction will increase
• catalysts provide an alternative pathway for a reaction that has a lower activation energy
• increasing the concentration increases the rate of reaction because there will be more particles in the same volume, so more frequent collisions
• the collision theory is the theory that chemical reactions only occur when particles collide with enough energy
• a dynamic equilibrium is the point in a reversible reaction where the rate of the forwards reaction is the same as the rate of the reverse reaction - in a closed system
• 5 factors that affect the rate of reaction: 1. temperature 2. surface area 3. concentration of solutions 4. pressure of gases 5. catalysts
• the effect of increasing the surface area increases the rate of reaction
• increasing surface area increases the rate of reaction because there are more particles available to collide, so more frequent collisions
• increasing concentration increases the rate of reaction
• the activation energy is the minimum amount of energy a particle needs to react with another particle when it collides
• if the temperature is increased in an exothermic forwards reaction, the backwards reaction will be increases because it is endothermic so, it will reduce the temperature
• increasing the temperature increases the rate of reaction because the particles have more energy, so they move faster and will collide more frequently, and more particles have the minimum energy needed to collide successfully
• Le Chatelier's principle is when a reaction at equilibrium is changed, it will seek to counteract that change
• increasing the temperature will increase the rate of reaction
• the amount of product doesn't change at equilibrium
• increasing pressure of a gas increases the rate of reaction because there are more particles in the same volume, so more frequent collisions
• in an exothermic forward reaction, the reverse direction will be endothermic