Answer:
The correct answer is The forward reaction is favored.
Explanation:
A reaction has a chemical equation given by the following:
Reactants ⇆ Products
The forward direction is from reactants to products and the reverse direction is from products to reactants.
The equilibrium constant K is calculated from the concentrations of reactants and producst at equilibrum as follows:
[tex]K = \frac{[Products ]}{[Reactants ]}[/tex]
If K is higher than 1, that means that the concentration of products at equilibrium are higher than the concentration of reactants at equilibrium:
[Products] > [Reactants]
Thus, the forward direction of the reaction os favored (from reactants to products).
