Earlier in this unit, K was defined as the equilibrium constant. In this unit, we are going to define the Kp. The Kp is the equilibrium constant using pressure. When using Kp, we don't use concentration, instead we use the partial pressures of each substance. (Note: the only substances put int the equilibrium constant when using pressures are gases.) So, the rule for the equilibrium constant with pressure is:
for the reaction of:
The relationship between K and Kp is:
where R is .08206 L * atm / (K * mol) T is the temperature in Kelvin delta n is the difference between the gaseous mole of product and the gaseous moles of the reactants
Right now, you are probably saying, FINALLY we get to use the equilibrium constant. Well you are right. Now you get to see how all the pieces of the puzzle fit together. First, when we know the equilibrium constant, we can determine if the equilibrium will have more product or reactants in it. If the K is less that 1, the the equilibrium position will probably contain a lot of reactants. If the K is greater that 1, then the equilibrium position will probably contain a lot of products.
Secondly, if you know to equilibrium constant and in the problem, they gave you all the concentrations or pressures you can calculate the reaction quotient (Q). The "Q" is exactly the same equation as you equilibirium constant, except the numbers that you put in is the concentrations or pressures that you were given in the equation. Once you have solved for the "Q", you can compare it to the equilibrium contant.
|Table of Contents:
Unit 7 - Section 2
Unit 7 - Section 4