I have the following equation at equilibrium :
HF = H+ + F- Kc = 6,7 x 10^-4
How do I know if the direct or the indirect reaction is favored?
Explanation from Alloprof
This Explanation was submitted by a member of the Alloprof team.
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To predict if the direct or the indirect reaction is favored, we must look at the value of the equilibrium constant (Kc).
When Kc is bigger than 1, the concentration of the products is bigger than the one of the reactants. Therefore, the direct reaction is favored.
When Kc is smaller than 1, the concentration of the reactants is bigger than the one of the products. Therefore, the indirect reaction is favored.
When Kc is almost equal to 1, there are as many reactants as products. Therefore, no reaction is favored.
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