CHEM102 Lecture Notes - Reaction Quotient, Ideal Gas Law, Equilibrium Constant

• School: University of Alberta
• Department: Chemistry
• Course: CHEM102
• Professor: Sai Yiu

Document Summary

Introduction: many physical / chemical processes are reversible. If the reversible process is in a closed vessel (neither the reactant nor the product can escape), a state of equilibrium will develop. Both the forward and reversed reactions are elementary steps and so, Rate (forward) = k (forward) [a]a x [b]b k (forward) = rate constant of the forward reaction. c c + d d a a + b b. Rate (reversed) = k (reversed) [c]c x [d]d k (reversed) = rate constant of the reversed reaction. Since at equilibrium, rate (forward) = rate (reversed) k (forward) [a]a x [b]b = k (reversed) [c]c x [d]d k (forward) / k (reversed) = [a]a x [b]b: kc is called the equilibrium constant and it is dependent only on the temperature, the ratio is called the equilibrium constant expression. In most cases, the values of k are shown as dimensionless numbers. This is because in thermodynamics, the concentration is expressed as the.