Chem – LESSON 18: Equilibrium

January 25th, 2012 |

Author: Andrew

This is one of the most difficult lessons for most students. Make sure you put a lot of effort into this lesson.

NOTE: None of the equilibrium constants ( K ) in this lesson are the true equilibrium constants of the formula. This is also the case for the Δ H of chemical equations and the thermodynamics. I made up both the equilibrium constants and the Δ H numbers because I did not want to spend hours searching for them. The fact that I made them up does not make any of my methods for solving these examples incorrect. Just don’t take the number you see here to be absolute truth. All of the numbers are created to guide you through the process of how to solve these problems.

What should you know before attempting this lesson?

If you have trouble in this lesson go back to sections on proportions and ratios, exponents, solving for an unknown, definition and layout of a chemical equation, states of matter in a chemical equation, coefficients, using stoichiometry in conversions, and Molarity.

New Learning Sections:

—> Equilibrium Definition

—> Products or Reactants Favored

—> Equilibrium Equations

—> Molar Concentration and the Equilibrium Constant Kc

—> College: The Relationship Between Different Equilibrium Constants

—> College: Pressure and the Equilibrium Constant Kp

—> College: Conversions Between Kc and Kp

—> Le Chatelier’s Principle: Moles or Concentration

—> Le Chatelier’s Principle: Temperature or Energy

—> Le Chatelier’s Principle: Volume and Pressure

—> College: Equilibrium for Acids and Bases