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
Likewise, an equilibrium constant that is greater than
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