Favoring Products/Reactants

[Jennifer Guzman 4C]

What does it mean when equilibrium favors either the products or reactants and what is the significance of a side being favored ?

[Tatum Keichline 2B]

If q is less than k, the reaction moves towards the products. If q is greater than k, the reaction moves towards the reactants. K is just equilibrium.

[Jane Burgan 1C]

If K is greater than 10^3, that means the products are favored - there is a higher concentration of products compared to that of reactants at equilibrium. When K is less than 10^-3, that means the reactants are favored - there is a higher concentration of reactants compared to that of products at equilibrium. When K is between 10^-3 and 10^3, then neither are favored.

[AdityaGuru1H]

basically since q is calculated the same way as k using conc[p]/conc[r], if q > k then that means that there is more product than there should be at equilibrium and the reaction will go towards the reactants and the reverse if q < k