Chemical equilibrium

• Le Chatelier's principle states that if an external factor changes, then the system will change so as to counteract this effect.
• Temperature affects the speed of reactions by increasing the kinetic energy of particles, leading to more collisions between them.
• The rate at which a chemical reaction occurs depends on several factors such as temperature, pressure, surface area, catalysts, and concentration.
• The position of the equilibrium lies to the left when the concentration of reactants is greater than that of products.
• The position of chemical equilibrium is determined by the relative rates at which forward and reverse reactions occur.
• If the rate of the forward reaction increases more than the rate of the reverse reaction, the position of equilibrium shifts towards products.
• If the rate of the reverse reaction increases more than the rate of the forward reaction, the position of equilibrium shifts towards reactants.
• Increasing temperature increases the rate of reaction until it reaches its maximum value (optimum), beyond which further increase in temperature decreases the rate of reaction due to decomposition or explosion.
• Catalysts are substances that can accelerate a reaction without being used up themselves.
• The optimum temperature is different for every chemical reaction.
• Increasing the temperature increases the frequency of successful collisions between reactant molecules, resulting in faster rates of reaction.
• Increasing the concentration of one side of the equation shifts the equilibrium towards the other side.
• Chemical equilibria


  Reversible reaction
• Reversible reaction


  A reaction that can go in both the forward and backward direction
• Reversible reaction is exothermic in one direction


  Endothermic in opposite direction
• Same amount of energy is transferred
• Equilibrium


  Forward and backward reaction will take place as exactly the same time
• System responds to the change
• when reaction reach equilibrium

  when the forward and backward reaction occurr at same rate. the concentration of product and reactant are equal and in close system
• Where the equilibrium position lay

  To the place where it has higher concentration
• Concentration of the product(s)

  Greater than the concentration of the reactants at equilibrium
• Effect of concentration

  Yea

  
• When we talk about pressure at eq

  It’s the yield of substance that changes not concentration
• If pressure increases

  Equilibrium moves to the side with fewer gas molecules
• Heating

  The process of adding heat to a system to increase its temperature. Can increase the reaction rate by providing energy to overcome the activation energy required for the reaction to occur.
• Cooling

  The process of removing heat from a system to decrease its temperature. Can decrease the reaction rate by removing energy from the system, which can slow down or stop the reaction.
• What is the Kc equation 


  Kc= [product 1] X [product 2]

  ———————————————

  [reactant 1] X [reactant 2]