Reaction Quotient

[Samantha Chung 4I]

As I was completing the reading section, I noticed that there was a "reaction quotient" - what is the difference between this sand the K value?

[Emma Scholes 1L]

K is used to describe a reaction at equilibrium. The reaction quotient is used to describe a reaction that is not at equilibrium. If the reaction quotient is equal to K, you know that the reaction is at equilibrium.

[Becky Belisle 1A]

The reaction quotient still has the same formula as the equilibirum constant, except for the equilibrium constant the values used are the ones at equilibrium.

[Chris Freking 2G]

K refers to the [P]/[R] ratio at equilibrium. Although Q also refers to the [P]/[R] ratio, it can be measured at any point in time in a reaction--including equilibrium.
If Q<K, then the forward reaction (products forming) is favored.
If Q>K, then the reverse reaction (reactants forming) is favored.
If Q=K, then the reaction is at equilibrium and reactants and products are being formed at equal rates.

[megan blatt 2B]

Going off of the previous comments, Q is the reaction quotient which is calculated the same way that K is. However, K is used once the reaction has reached equilibrium while Q is used for any other point in the reaction while it is reaching equilibrium.

[Jonny Schindler 1A]

Both K and Q represent the ratio of products to reactants, but using Q implies that the reaction is not at equilibrium and the ratio will shift until equilibrium is reached. At this point, the ratio is represented as K