The terms Q and K refer to reaction components at non-equilibrium and equilibrium conditions, respectively. For a forward reaction to be favored in a living cell, which of the following statements describes the relationship between Q and K?
a. The value of Q must be less than that of K.
b. The value of K must be less than that of Q.
c. No conclusion can be drawn about Q and K for a favorable process.
d. Cells are at equilibrium so none of the above statements is true

The value of Q must be less than that of K.

Explanation:

The difference of K and Q can be understood with the help of an example as follows

         A ⇄ B

In this reaction A is converted into B but after some A is converted , forward reaction stops At this point , let equilibrium concentration of B be [B] and let equilibrium concentration of A be [A]

In this case ratio of  [B] and  [A]  that is

K =  [B] / [A] which is called equilibrium constant.

But if we measure the concentration of A and B ,before equilibrium is reached , then the ratio of the concentration of A and B will be called Q. As reaction continues concentration of A increases and concentration of B decreases. Hence Q tends to be equal to K.

Q = [B] / [A] . It is clear that Q < K before equilibrium.

If Q < K , reaction will proceed towards equilibrium or forward reaction will

proceed .

The electrons of an atom, in particular valence electrons, are involved in chemical bonding.

Explanation: The reason is that the electrons are the most movable part of an element. The result of chemical bonding is that the two atoms share the electron density,