# Chapter 14 Outline

## 14.3 The Equilibrium Constant (K)

The general equation for equilibrium constant (K)

For a reaction aA + bB <--> cC + dD ## 14.4 Expressing the Equilibrium Constant in Terms of Pressure

When equlibrium is calculated using concentration, use Molarity. When equlibrium is calculated using pressure you must be consistent about which units are used. The textbook says pressure should be in atm, but it can be in any unit as long as you are consistent. You can convert between Kc and Kp using the ideal gas law and the change in moles of gas from reactant to product so that:

Kp = Kc(RT)delta_n

## 14.5 Heterogeneous Equilibrium: Reactions Involving Solids and Liquids

Solids and pure liquids have constant concentration - as long as they are present, so they are not included in the equlibrium expression - they are already part of the constant.

## 14.6 Calculating the Equilibrium Constant from Measured Equilibrium Concentrations

The general equation for equilibrium constant (K)

For a reaction aA + bB <--> cC + dD ## 14.7 The Reaction Quotient: Predicting the Direction of Change

q is calculated using the same equation as K - but it is NOT at equlibrium. You can use this to predict the direction of the reaction, since q will go to K as the system goes to equlibrium.

## 14.8 Finding Equilibrium Concentrations

Learn how to use the Initial, Change, Final table. You MUST be able to solve these problems.

## 14.9 Le Chatelier's Principle: How a System at Equilibrium Responds to Disturbances

This principle lets you predict the effect of changing concentration, temperature, and volume on an equlibrium system.