**The Equilibrium Constant (K**_{eq}) **What is an
equilibrium constant?**

At equilibrium, all the concentration of reactant and products are constant. We use
the concentration to calculate the equilibrium constant.

**equilibrium constant (K**_{eq}) - The product of the molar concentrations
of the products for a chemical reaction, each raised to the power of its respective
coefficient in the equation, divided by the product of the molar concentrations of the
reactants, each raised to the power of its respective coefficient in the equation.

*This might seems pretty confusing right now, let's look at some examples and see how
we can use this equilibrium constant.*

The equation for equilibrium constant is:

where,

**Notice a few rules**,

1. [A], [B], [C], and [D] = molar concentration at equilibrium.

2. products are always in the numerator, and reactants are always in the denominator.

3. coefficients in the chemical equations are the exponents.

4. Solids and liquids are ignored.

5. No units for K_{eq
}6. Concentrations are always in moles per liter.

*Example: *What is the equilibrium constant expression for ?

In this case, notice that H_{2}O is in the gaseous form. If it was in the liquid
or the solid state, then we won't use it in the K_{eq}.

After putting everything into the equation, we get the answer:

_{}

*Example: *What is the equilibrium constant expression for ?

This is slightly different than the above example. In this case, there is a solid in the
equation. Looking back at rule #4; we will need to omit the solid from the equilibrium
expression.

- Note that the value of the equilibrium constant depends on the temperature. If the
temperature change, then the concentration will change also. Thus we will have a different
*valve*. (The equation for the equilibrium constant is still the same).

**How to calculate the value of an equilibrium constant?**

Once we have the equilibrium constant expression from the chemical equation. We can
just plug in the molar concentrations at equilibrium to get the value of the equilibrium
constant.

*Example:* At the temperature 400^{°} , the equilibrium molar
concentrations are:

[CO] = 0.613

[H_{2}] = 1.839

[CH_{4}] = 0.387

[H_{2}O] = 0.387

for the reaction

What is the value of the equilibrium constant?

*Step 1:* We have to first figure out the equilibrium constant expression.

Which is:

*Step 2:* Plug in the numbers and solve:

= 0.0393 (notice there is no unit)

To sum it all up, the equilibrium constant gaves the relative amounts of products and
reactants at equilibrium. We can use this number to figure out all sorts of questions
related to equilibrium.