# Question #28ef9

##### 1 Answer

#### Explanation:

The **equilibrium constant** is defined as the ratio between the product of the *equilibrium concentrations of the products* raised to the power of their respective stoichiometric coefficients and the product of the *equilibrium concentrations of the reactants* raised to the power of their respective stoichiometric coefficients.

This basically tells you that an equilibrium constant that is **smaller than** **reactants are favored**.

Likewise, an equilibrium constant that is **greater than** **products are favored**.

You can thus say that the *higher* the value of

In your case, you have

#K_c = 9.3 * 10^(-13)#

#K_c = 3.6 * 10^(20)#

#K_c = 2.0 * 10^9#

So, you know that the higher the value of

#9.3 * 10^(-13) " "< " "2.0 * 10^9 " " < " "3.6 * 10^(20)#

For

#K_c = 9.3 * 10^(-13)#

you will have more reactants than products at equilibrium, i.e. the reverse reaction will be favored.

For

#K_c = 2.0 * 10^9" " and " " K_c = 3.6 * 10^(20)#

you will have more products than reactants at equilibrium, i.e. the forward reactions will be favored.

The difference in magnitude between the two values implies that for **significantly more of the reactants** to products than for