The given statement is TRUE.
When the rate of the forward reaction equals the rate of the backward reaction, this is known as an equilibrium reaction.
The ratio of the product of the concentration of the products to the product of the concentration of the reactants, each elevated to their stoichiometric coefficient, is known as the equilibrium constant.
As in the case of the specified equilibrium reaction;
[tex]2H_{2} O(g)[/tex]⇆2H[tex]_{2}[/tex](g)+[tex]O_{2}[/tex](g)
[tex]K_{eq} =\frac{(H_{2})^{2} (O_{2})_}[/tex]/ [tex](H_{2}O)[/tex]
A number that reflects a reaction's equilibrium is known as the equilibrium constant. When the reaction achieved equilibrium, it became a reaction quotient.
If Keq is higher than 1, the majority of the combination is made up of the products. If Keq is greater than 1, on the other hand, the mixture does not include the reactants. The equilibrium in this situation is to the left or toward the reactants.
Learn more about equilibrium constant.
https://brainly.com/question/19340344
#SPJ4
