Equilibrium

[smurphy1D]

What is the difference between Q and K?

[Veronica_Lubera_2A]

K is when the reaction reaches equilibrium. Q is a specific point in time before reaching equilibrium. We often compare Q to K; for example if Q<K then the reaction will shift to the right.

[Michael Nguyen 1E]

Q and K are calculated in the same way by using the same equation. However, K is a constant that is calculated using the concentrations when the reaction reaches equilibrium while Q changes as the reaction proceeds. Often, we compare Q and K to determine which direction the reaction will continue over time.

[Qiu Ya Wu 4I]

Q is known as the reaction quotient and K is known as the equilibrium constant. One important thing to note is that K stays constant for a specific reaction at a specific temperature while Q does not have a predetermined value.

[Kavya Immadisetty 2B]

Although Q and K are calculated the same way, the difference is the state of the reaction at the time when this is calculated: Q can be any specific point of time while K must be when the reaction is at equilibrium.

[Caroline Zepecki]

Q is the constant of concentration at any point during the reaction, whereas K is the constant of concentration at equilibrium.

[KBELTRAMI_1E]

Q is just used to compare to K in order to determine which reaction will proceed (toward product or reactant).

[Hailey Kim 4G]

K is the equilibrium constant, while Q is the reaction quotient. They are calculated the same way but you can compare Q and K to determine if the forward reaction or the reverse reaction is favored. If Q<K at some time during the reaction, then reactants are favored. If Q>K at some time during the reaction, then products are favored.