RATES OF EQUILIBRIUM REACTIONS

1. Forward reactions occur first because no products have formed yet.
   
2. As products form, they may again react to form initial reactants. When the rate of the products forming equals the rates the reactants are re-forming, the system is in a state of dynamic equilibrium.
   
3. In essence, forward reactions occur more quickly in the beginning to form products.
   
4. Reverse reactions start off slowly because they must wait for products to form.
   
5. Eventually, both the forward and reverse reactions equal out.
   
6. The Effect of Surface Area on Reactions: The more finely divided the solid is, the faster the reaction happens. A powdered solid will normally produce a faster reaction than if the same mass is present as a single lump.
   **(Go to http://www.youtube.com/watch?v=srKewy69Pdk for a video on how SURFACE AREA affects the rate of reaction!)
   
   



7. The Effect of Concentration on Reactions: As the concentration of the reactions decreases, the forward reaction slows. As the concentration of the products increase, the reverse reaction speeds up.
   **(Go to http://www.youtube.com/watch?v=srKewy69Pdk for a video on how SURFACE AREA affects the rate of reaction!)
   
8. The Effect of Temperature on Reactions: As you increase the temperature the rate of reaction increases. As a rough approximation, for many reactions happening at around room temperature, the rate of reaction doubles for every 10°C rise in temperature.
   **(Go to http://www.youtube.com/watch?v=0XQVXFL4uoo for a video on how TEMPERATURE affects the rate of reaction!)
   
   


9. Eventually the rates of reaction for the forward and the reverse process equal out!

**Example:

CH4 + H2O ⇌ 3H2 + CO

(In this reaction, as the CH4 and water get "used up," more products form and the forward reaction slows. As the products form, there is now the potential for the reverse reaction. As more and more product form - meaning, as the concentration of product increases - the reverse reaction speeds up.