Q & K
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Re: Q & K
Q and K are different. Q is the reaction quotient, which takes the concentrations of products divided by the concentration of reactants when the reaction is not at equilibrium. K is the equilibrium constant, which takes the concentration of products at equilibrium divided by the concentration of reactants at equilibrium. When a reaction is at equilibrium, K stays the same.
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Re: Q & K
Adding to the answers above, K always stays the same unless the temperature changes. Q is what changes when the reaction moves away from equilibrium.
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Re: Q & K
When studying a reaction at a specific temperature, the Q we calculate will equal the K value corresponding to that temperature when the reaction reaches dynamic equilibrium, that is, when the ration of products and reactants are the same for Q and K.
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Re: Q & K
Q = K only when reaction is at equilibrium.
If Q is calculated at the same temperature as K then they can equal each other. K is a constant so it always stays the same at the same temperature. Q can also be smaller or bigger than K, which proves that the products or reactants are favored, respectively.
If Q is calculated at the same temperature as K then they can equal each other. K is a constant so it always stays the same at the same temperature. Q can also be smaller or bigger than K, which proves that the products or reactants are favored, respectively.
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Re: Q & K
No, Q only equals K when the reaction is at equilibrium. When the reaction is not at equilibrium, Q will be smaller or larger than K.
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Re: Q & K
Most of the time, Q and K are different. Q can be calculated at any time in the reaction while K is calculated at equilibrium. When the reaction is at equilibrium, Q=K.
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Re: Q & K
While Q can equal K, this is not true all of the time. If Q is equal to K, that means that a chemical reaction is in equilibrium. However, if Q is greater than or less than K, then the reaction is not in equilibrium.
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Re: Q & K
K is constant (at a constant temperature) for a certain reaction. If you were performing that same reaction at that temperature, the current proportion of products/reactants is Q. Once equilibrium is achieved, Q = K.
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Re: Q & K
While it is possible for Q to equal K (when the reaction is at equilibrium), this is not the case most of the time.
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Re: Q & K
I think of K as the general equilibrium constant for any chemical reaction, while Q is the specific equilibrium value for any amounts of reactant and product.
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Re: Q & K
No Q does not equal K. Q is basically the ratio of the products to reactants any time the system is NOT at equilibrium while K is when it IS at equilibrium.
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Re: Q & K
Q only equals K when the reaction is at equilibrium. If the reaction is not at equilibrium then Q must be greater than or less than K but never equal to.
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Re: Q & K
K is when the reaction is at equilibrium and Q is whatever it is at its current state whether it is in equilibrium or not. Q equals K when the reaction is at equilibrium. Q can change but K cannot. For example, if a reaction is at equilibrium then the Q and K will be equal but if the concentrations are changed, the Q will change but the K will not and it is no longer at equilibrium
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