Quotient

[Matthew Lee 3L]

Is Q basically the same thing as K or are they different?

[Nehal Banik]

Q itself, is the reaction quotient for the reaction given with whatever initial numbers that you are given. Whereas K is the equilibrium quotient, which is the ratio of the concentration/partial pressure of the products and reactants.

[Lily Guo 1D]

Q is the reaction quotient, while K is the equilibrium quotient. They both follow the same expression -- the product of the concentrations or partial pressures of each product raised to the power of its stoichiometric coefficient over the product of the concentrations or partial pressures of each reactant raised to the power of its stoichiometric coefficient. However, when calculating Q, you can use the concentrations or partial pressures of the reactants and products at any point in the reaction. When calculating K, you use the equilibrium concentrations or partial pressures, not just any concentrations or partial pressures.

[aaron tang 2K]

Q is the quotient which is the for when the reaction is given with whatever initial values are given. K is the equilibrium quotient which is the ratio of the concentration and partial pressure of the reactants and products

[Victor Qiu 1C]

Basically, K is the relative ratio of products to reactants when the reaction is at equilibrium, while Q is the relative ratio of products to reactants at a given instant (the reaction might not be at equilibrium).

[Jessica Katz]

Q is the relative concentrations at a given time, and k is only used when at equilibrium. so they are used in comparison to determine if more products or more reactants are going to be made in order for the Q to equal K.

[Daniela Santana 2L]

Q is the reaction quotient, K is the equilibrium constant. Q can be calculated at any time whereas K can only be calculated at equilibrium. Hope this helps!

[Simran Bains 2C]

Q is the reaction quotient, whereas K is the reaction quotient at equilibrium specifically.

[Griffin G]

Q is calculated the same way as K, just when the system is not at equilibrium.

[Hannah Lechtzin 1K]

Q and K are almost the same. The only difference is the K is when the reaction is at equilibrium while Q is not.

[rhettfarmer-3H]

Q is basically K at a time of the reaction that is not an equilibrium. Use the term Q to basically indicate that it is not at equilibrium. Therefore, they are entirely the same, it helps to describe the state of the reaction.

[SashaAnand2J]

Hi Matthew!

Q is similar to K, in that the equation setup for both are identical, however, the concentrations that are substituted into the equations are different. Q is when the concentrations of the reactant and product are not at equilibrium. K always uses equilibrium constants.

[Carly_Lipschitz_3H]

K is the equilibrium constant, and Q is the reaction quotient. They are both calculated the same way, but K stays constant. Q does not stay constant since it can be taken at any time. Q doesn't specifically need to be taken when the reaction is at equilibrium like K is. When Q<K, the forward reaction is favored, and when Q>K, the reverse reaction is favored.