BIOCH499A Study Guide - Sulfur Trioxide, Phosphorus Pentachloride, Reaction Quotient

• School: University of Alberta
• Department: Biochemistry
• Course: BIOCH499A
• Professor: Gail Amort- Larson

Document Summary

Last time we had as an example the hydrogenation of unsaturated organic molecules. Give it a try under simulated conditions: 45 min, closed book, etc. In a sealed flask at room temperature both exist together. The amounts of each gas in the flask are dictated by the equilibrium constant. All chemical reactions reach a state of equilibrium. That is, they reached a state in which reactants are left, products are present but nothing seems to be happening. Reaction is continuing on the microscopic level, but the rate at which the products are formed, equals exactly to the rate at which reactants are formed, so there is no. Net change. k1 [reactants]stoich coefficients = k 1 [products]stoich coefficients (products = reactant of the reverse reaction) K = equil. constant = k1 k 1. Constant is capital k, rate const. is small k. When the concentrations are constant, the rxn is at equilibrium.