Reversible reactions

• If the forward reaction is exothermic in the backwards reaction will be endothermic
• Energy is conserved during chemical reactions. The energy, absorbed or released by the forward reaction will be exactly equal to the energy, absorbed or released by the backwards reaction.
• When reversible reactions happen within a close system, a dynamic equilibrium will eventually be reached
• A close system is when the reactants and products can’t be added or removed. Remove
• at dynamic equilibrium, the right of forward and backwards reactions are equal, and the concentration remains constant
• Le Chateliers principle: If a system is at equilibrium, a change in the conditions will cause the equilibrium position to shift to counteract the change
• Changing the temperature for a reaction at equilibrium will take it out of equilibrium. If you decrease the temperature, it will shift into the exothermic direction. If the temperature is increased, then the position will shift to endothermic.
• Pressure changes only affect reactions that involve gases. If you decrease the pressure, then the positional shift to favour the reaction that produces the most gas molecules
• If you increase the reactants concentration, then the equilibrium will shift to the products
• When reversible reactions happen within a closed system a dynamic equilibrium will be reached