10: Equilibrium
- Page ID
- 235982
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- 10.1: The Rate of a Chemical Reaction
- The rate, or speed, at which a reaction occurs depends on the frequency of successful collisions. Remember, a successful collision occurs when two reactants collide with enough energy and with the right orientation. That means if we can do things that will increase the number of collisions, increase the number of particles that have enough energy to react and/or increase the number of particles with the correct orientation we will increase the rate of a reaction.
- 10.2: The Idea of Dynamic Chemical Equilibrium
- Some reactions are reversible, meaning the reaction can go backwards in which products react to form reactants. If the forward and reverse reactions are happening at the same rate, the reaction is said to be at equilibrium or dynamic equilibrium. At this point, the concentrations of reactants and products are not changing (or are constant) and we would see no difference in our reaction container. However, reactions are still occurring in both directions.
- 10.3: The Equilibrium Constant - A Measure of How Far a Reaction Goes
- In the previous section, you learned about reactions that can reach a state of equilibrium, in which the concentration of reactants and products aren't changing. If these amounts are changing, we should be able to make a relationship between the amount of product and reactant when a reaction reaches equilibrium.