Q and K

[Sean Phen]

What are the differences between Q and K?

[Selena Quispe 2I]

K is the equilibrium constant and Q is the reaction quotient, which is calculated the same way you would calculate the equilibrium constant however the reaction quotient is not at equilibrium. When comparing the equilibrium constant and reaction quotient if Q is larger than K then you have too many products and the reaction will favor the formation of reactants. If your Q is less than K then you have too many reactants and the reaction will favor the formation of products. I hope this helps!

[AlbertGu_2C]

Q and K are very similar, with the difference being that K is ONLY at equilibrium, while Q can be at any point during the reaction, including equilibrium

[Levon Grigoryan]

Q = [B]/[A]. K = [B]equalibrium/[A]equalibrium

This is the simple way I remember it, so the wording does not get confusing. I think this is more simple.

[LovepreetSran_3H]

K is only at equilibrium, and Q is at any particular point of the reaction.

[Kelly Ha 1K]

Q is the reaction quotient, or the amount (in terms of concentration or partial pressures) of products over the amount of reactants at any point in the reaction. K is the equilibrium constant, which is calculated the same way as Q and is essentially Q at equilibrium.

[Heather Costa 2C]

k is for the equilibrium constant and Q is for the reaction quotient they are essentially the same at equilibrium

[Kiara Phillips 3L]

K is the equilibrium constant and Q is the constant of a system when not at equilibrium and the value of Q can tell us which way the reaction is proceeding etc. Basically Q is K when we have not yet found K. Hope this helps!

[Caitlin_Doak_2H]

Q is the chemical quotient and it is the result if the equation is not in equilibrium. When it is, it is K

[Arjan G 2H]

Hi! K is usually a more broad term for either Kc or Kp, and this represents the equilibrium of a chemical equation. The variable Q is more general and represents the reaction quotient of a chemical equation based on the concentrations of the products and reactants. This means that for any chemical equation, while under the same conditions, it can only have 1 Kc value, and numerous Q values, as there is only one point where the system can be at equilibrium. I hope this helps!

[Jessica Cornelia Hongarta 1G]

Hi! So, K (equilibrium constant) is the constant of the reaction when it is at equilibrium while Q is the reaction quotient at any stage of the reaction (does not have to be at equilibrium).

[Kimberly_martinez2I]

K is equilibrium constant and Q is the reaction quotient. They are calculated in the same way.

[Amy Kalteis 2F]

In addition to the other answers, I just want to add that if a reaction is at equilibrium, there is no difference between Q and K! They are at the same value.

[Mia Hansen 2I]

Q is the reaction quotient (calculated at any given time during a reaction) and K is the equilibrium constant (calculated at equilibrium). Finding Q and comparing it to K can tell you which way a reaction is going to proceed. Forward is favored: Q is less than K. Reverse is favored: Q is larger than K. (Both directions are still occurring just not equally)

[Isabelle Rieke-Wey 2G]

Hi!
Q is the reaction quotient, which is calculated at any time during the reaction, while K is the equilibrium constant, which is calculated when the reaction is at equilibrium. When you compare the two, this can tell you which way the reaction is going to shift.

[Sean Sanders 1E]

Q and K are similar to one another and use the same formula of [products]/[reactants]. The concentrations for K are those at equilibrium while the concentrations for Q can be during any point during the reaction.

[Lawrence Tran 2H]

Q and K are both calculated as [products]/[reactants]. If Q < K, than the formation of products is favored, while if Q > K, the formation of reactants is favored.