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# Calculations of Free Energy and Keq

## Demonstrates equations used to relate free energy and equilibrium constants.

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Calculations of Free Energy and Keq

Credit: User:Bothar/Wikipedia
Source: http://commons.wikimedia.org/wiki/File:WonderCaves_Stalagmites.JPG

What are these formations called when they point down?

Formation of stalactites (pointing down) and stalagmites (pointing up) is a complex process. Solutions of minerals drip down and absorb carbon dioxide as water flows through the cave. Calcium carbonate dissolves in this liquid and redeposits on the rock as the carbon dioxide is dissipated into the environment.

### Equilibrium Constant and

At equilibrium the  for a reversible reaction is equal to zero. relates the concentrations of all substances in the reaction at equilibrium. Therefore we can write (through a more advanced treatment of thermodynamics) the following equation:

The variable  is the ideal gas constant (8.314 J/K • mol),  is the Kelvin temperature, and  is the natural logarithm of the equilibrium constant.

When  is large, the products of the reaction are favored and the negative sign in the equation means that the  is negative. When  is small, the reactants of the reaction are favored. The natural logarithm of a number less than one is negative and so the sign of is positive. The Table below summarizes the relationship of  to :

 Description >1 positive negative Products are favored at equilibrium. 1 0 0 Reactants and products are equally favored. <1 negative positive Reactants are favored at equilibrium.

Knowledge of either the standard free energy change or the equilibrium constant for a reaction allows for the calculation of the other. The following two sample problems illustrate each case.

#### Sample Problem: Gibbs Free Energy and the Equilibrium Constant

The formation of nitrogen monoxide from nitrogen and oxygen gases is a reaction that strongly favors the reactants at 25°C.

The actual concentrations of each gas would be difficult to measure, and so the  for the reaction can more easily calculated from the , which is equal to 173.4 kJ/mol.

Step 1: List the known values and plan the problem.

Known

Unknown

In order to make the units agree, the value of will need to be converted to J/mol (173,400 J/mol). To solve for , the inverse of the natural logarithm, , will be used.

Step 2: Solve.

The large positive free energy change leads to a value that is extremely small. Both lead to the conclusion that the reactants are highly favored and very few product molecules are present at equilibrium.

#### Sample Problem: Free Energy from

The solubility product constant  of lead(II) iodide is 1.4 × 10-8 at 25°C. Calculate  for the dissociation of lead(II) iodide in water.

Step 1: List the known values and plan the problem.

Known

Unknown

The equation relating  to  can be solved directly.

Step 2: Solve.

The large, positive  indicates that the solid lead(II) iodide is nearly insoluble and so very little of the solid is dissociated at equilibrium.

#### Summary

• The relationship between  and  is described.
• Calculations involving these two parameters are shown.

#### Practice

Questions

1. What is the difference between and ?
2. At equilibrium, why does the equation between free energy and equilibrium constant reduce to ?
3. What other equilibrium units could we use?

#### Review

Questions

1. When  is large, what will be the sign of ?
2. When  is small, are reactants or products favored?
3. What does  stand for?