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Slide 1

• Reversible reactions
• Are when reactions go in both forward and backward reactions.
• Forward reaction
• Initially reactants are used up quickly but then slow down as their concentration drops.
• Backwards reaction
• Initially reactants are reformed slowly, but then speed up as the concentration of products increases.
• At this point, the rate of the forward reaction equals the rate of the backward reaction. This=Dynamic Equilibrium.
• The concentration of each substance remains constant.

Slide 2

• LCP
• If a reaction at equilibrium is subjected to a change in concentration, pressure or temperature, the position of equilibrium will move to counteract the change.
• Changing conc.
• If we increase the concentration of a reactant or product the equilibirum will shift to try to reduce the concentration.
• If we increase the concentration of reactants, the equilibrium will shift to the right to use it up and reduce the concentration, and more product will be produced.
• If we decrease the increase the concentration of product, the equilibrium will shift to the left to try and use it up and reduce the concentration. More reactant will be produced.
• This only works in homogeneous equilibria.

Slide 3

• If we increase the pressure, the equilibrium will shift to try and reduce the pressure.
• If we increase the pressure, equilibrium will shift to the side with the fewest moles, reducing the pressure, and more product will be produced.
• If we decrease the pressure, equilibrium will shift towards the side with more moles, increasing the pressure, and more

Slide 4

• LCP: If a reaction at equilibrium is subjected to a change in concentration pressure or temperature, then the position of equilibrium will move to counteract the change.
• If we increase the temperature, the equilibrium will try to reduce the temperature.
• If we increase the temperature, equilbirium will shift in the endothermic direction, reducing the temperature.