CHEM 134 Lecture Notes - Lecture 10: Ideal Gas Law, Equilibrium Constant

• School: University of Maryland
• Department: Chemistry and Biochemistry
• Course: CHEM 134
• Professor: Jason Kahn

Document Summary

Reversible reactions do not go to completion. They can occur in either direction. Chemical equilibrium exists when two opposing reactions occur simultaneously at the same rate. Systems can reach equilibrium when reactants have not converted completely to products. In the case grxn is < go rxn state with both reactants and products present is more stable than complete conversion. Products favored 103 > k > 10-3 reactants favored. Values of k greater than 103 indicate a strong tendency for reactants to form products, so equilibrium lies to the. Right, favoring the formation of products (kf >>kr) Values of k less than 10 3 indicate that the ratio of products to reactants at equilibrium is very small; reactants do not. Tend to form products readily, and equilibrium lies to the left, favoring the formation of reactants (kf<