Q vs. K

[Jose Robles 1D]

Need clarification, what is the distinction or similarities between the two?

[stephaniekim2K]

K is the constant at equilibrium while Q is the constant at any point in the reaction.

[Jose Robles 1D]

K is the constant at equilibrium while Q is the constant at any point in the reaction.

Cool thanks!

[alex_4l]

Q and K are similar in the sense that they are calculated the same way with products divided by reactants. They are different however with K being the equilibrium constant and Q being the reaction quotient. Q happens at any time during the reaction and K is the overall equilibrium

[Brianna Becerra 1B]

They are similar to each other as the calculation of products divided by reactants is the same. The main difference is that k occurs at equilibrium while q occurs before equilibrium is reached. By calculating Q and comparing it to K, we can tell which way the reaction is going more towards.

[Kishan Shah 2G]

Q and K are calculated using the same rules and formula. However Q is used when you are given initial concentration/pressure values, and K is used when you are given equilibrium concentration/pressure values. You can compare Q and K to determine in which direction the reaction will proceed.

[Sean Tran 2K]

Q and K are both calculated similarly, but Q can be calculated at any time during the reaction and can be compared with K to determine the direction in which the reaction is favored.

[Veronica Lu 2H]

Both are calculated using the same formulas but Q is used anytime during the reaction whilst K is calculated with equilibrium concentration and values!

[Shrayes Raman]

Q is basically calculated the same way as K but can be calculated at any point in a reaction not just during equilibrium

[SimranSangha4I]

Q is the constant through the entire equilibrium while K is the constant at equilibrium!

[Angela Wu-2H]

Q is focused on the reactants and products that are gasses or aqueous solutions, meanwhile K can be for all forms including solids I believe.