CHEM 102 Chapter Notes - Chapter 16: Inert Gas, Endothermic Process, Reaction Quotient

• School: Drexel University
• Department: Chemistry
• Course: CHEM 102
• Professor: King Daniel

Document Summary

16. 4 expressing the equilibrium constant in terms of pressure. Kp = kc(rt)delta(n: if the total number of moles of gas is the same before and ater the reacion, N = 0 and kp = kc units for k are usually omited. 16. 5 heterogeneous equilibria: reacions involving solids and liquids solids and pure liquids (water) are not included in the equilibrium expression because their concentraions do not change throughout the reacion. Mathemaical changes to k (hess" law: reversing the reacion inverts k (1/k, changing the coeicients raises k to an exponent (kmuliplier) Inding equilibrium concentraions from the equilibrium constant and all but one of the equilibrium concentraions of the reactants and products: rearrange the equilibrium constant equaion to solve for the unknown concentraion. 16. 9 le chatelier"s principle: how a system at equilibrium responds to disturbances. Le chatelier"s principle: when a chemical system at equilibrium is disturbed, the system shits in a direcion that minimizes the disturbance.