Difference between K and Q?

[Diana Chavez-Carrillo 2L]

The reaction quotient (Q) formula looks very similar to the formula used for the equilibrium constant, K so what is their difference? Is it just that K has to be at equilibrium or is there other differences between them?

[Samuel G Rivera - Discussion 4I]

Q and K have the exact same formula. Q can be any value depending on the state of the reaction. K is Q when the reaction reached equilibrium.

[Jamie Hwang 2F]

Yeah, K is at equilibrium while Q is at any stage of the reaction.

[205405339]

K represents the concentrations at equilibrium whereas Q represents concentrations not at equilibrium

[AKhanna_3H]

Q and K are both measured by the ratio of products over reactants, but K represents that ratio at equilibrium while Q can represent that ratio at any point in the reaction.

[905373636]

K is a fixed value for the reaction, while Q varies if the reaction is/is not yet at equilibrium and we can compare the two values to determine if the reaction is at equilibrium or not.

[Emma Joy Schaetz 1E]

Is the formula always the same for Q and K? I know whether we use Q or K depends on the equilibrium status of the reaction, but we find the values the exact same way otherwise?

[vibha gurunathan 1h]

The formula's the same and you find it in the same way, but you use current concentrations/pressures for Q and equilibrium concentrations/pressures for K.

[EthanPham_1G]

K is the equilibrium constant and can only be solved for when the concentrations of reactants and products at equilibrium are known. Q is the reaction quotient and can be solved at any point in the reaction, regardless if it is in equilibrium. If Q<K then the reaction moves forward and favors the products. If Q>K then the reaction moves reverse and favors the reactants.

[Alexandra Bartolome 2H]

Q is calculated the same was as K. However, K is the equilibrium constant while Q is the reaction quotient at any time during the reaction. You compare Q to K in order to find out whether the reaction is at equilibrium or not. When Q<K, the forward reaction is favored since the concentration of reactants is higher than the concentration of products. When Q>K, the reverse reaction is favored. If Q=K, the reaction is at equilibrium.

[Andres Merlos 2L]

They look very similar because the only difference between the two constants is when you should use them. You use K when the reaction is at equilibrium, and you use Q at any stage of the reaction. You can compare the two constants to determine which way the reaction is shifting.

[Lauren Stack 1C]

Q and K are actually calculated using the same formula with products over reactants. The difference between the two lies in when they apply. K ONLY applies to when a reaction has reached equilibrium. On the other hand, Q can represent any time during a reaction. Using Q, you an determine if the reaction is at equilibrium (K=Q) or what direction the reaction is moving in depending on if K>Q or K<Q.