K Vs Q Chem

The main difference between k and q is that k describes a reaction that is at equilibrium whereas q describes a reaction that is not at equilibrium.

K vs q chem. So k c for concentration and k p for pressure. If q k forward reaction is favoured. When this is the case and all values are given in pressures we use k p which is the equilibrium constant for pressure. 1 a a b b c c d d.

Q is used to determine whether or not the reaction is at an equilibrium. Q is a quantity that changes as a reaction system approaches equilibrium. Q 6 09 k another way to say this is that as long as the value of q is less than the value of k then the reaction proceeds in the forward direction. 7 q 12 so q k.

K is the numerical value of q at the end of the reaction when equilibrium is reached. 4 no it is not at equilibrium. Reaction proceeds in the forward direction. And k is 14 5 so we ll say it s somewhere around here.

It is important to understand the distinction between q and k. The reaction will shift to the right. Since q k the reaction will shift to the right to reach equilibrium. You use q when you are unsure if a reaction is at equilibrium.

At any given point the reaction may or may not be at equilibrium. For a given general chemical equation. By calculating q products reactants you can compare it to the k value products reactants at equilibrium to see if the reaction is at equilibrium or not. To determine q the concentrations of the reactants and products must be known.

So what s gonna happen is in order to reach equilibrium our concentrations are going to shift to the right to get q closer to k. So q we can put on our number line is somewhere around here. 6 q 32 0 so q k. The reaction will shift to the left.

We can see that q is less than k on our number line. So this is our q and this is our k. 5 q 0 033 so q k.