C6~The rate of chemical change

• FACTORS Affecting the rate of reactions:

  1)Temperature= as the temperature increases the particles gain more kinetic energy allowing them to move faster and therefore increase rate of reaction. When particles collide, they do so with more energy so the frequency of successful collisions increases.
• 2)Concentration=at higher concentration there are more particles in the same amount of volume, which means the frequency of collisions increases and therefore reaction is more likely to happen.
• 3)Surface area to volume ratio=an increase in surface area means more particles are exposed to other reactants and is a greater chance of particles colliding, which leads to more successful collisions per second.
• 4)Catalysts=using a catalyst lowers the activation energy meaning more particles have the minimum energy needed for a reaction to occur when they collide.
• DEFINE dynamic equilibrium:

  is the point at which the forward reaction occurs at the same rate as the backwards reaction in a reverse reaction in a closed system and there is no overall effect
• Le Chatelier's Principle:

  In 1884, he theorised that if the conditions of a reversible reaction at dynamic equilibrium was changed, the system would try counteract that change.- this means changing the conditions of the reaction can affect the yield of the reaction.
• If we increase the pressure on a reversible reaction at dynamic equilibrium, then the number of gas molecules will increase. This causes an imbalance between the numbers of gas molecules and solid/liquid molecules. The system tries to restore balance by increasing the rate of the forward reaction (which produces more gas molecules).