When Q=K
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When Q=K
Just for clarification, when Q=K, is it safe to assume that the reaction is at equilibrium?
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Re: When Q=K
Yes, if you start out solving for Q because you are unsure whether a reaction is at equilibrium, and then find that the value you calculate is equal to K, then you now know the reaction is at equilibrium.
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Re: When Q=K
Yes, if the Q (reaction quotient) value that calculates the ratio of product to reactant concentration is equal to the K (equilibrium constant) value, then the reaction is at equilibrium.
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Re: When Q=K
Hi, if Q=K, then the system is at equilibrium since the concentration of product over reactant is equal to the equilibrium constant K. Hope this helps!
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Re: When Q=K
Yes, since Q is the ratio of products to reactants, if that ratio is equal to K, then you can assume rxn is at equilibrium
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Re: When Q=K
Yes. This question is relevant when we are studying a reaction. We can compare a given K value to the a Q value based on the information we have of the reaction (concentration of products and reactants) in order to determine if the reaction has reached equilibrium or if it has not, which side of the reaction will it favor.
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Re: When Q=K
Yes essentially Q is used as a measure to see if the reaction has reached equilibrium, so once Q=K then we can confirm that the reaction is at equilibrium.
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Re: When Q=K
Q is the product to reactant ratio at any given time in a reaction while K is the product to reactant ratio at equilibrium. When Q=K, then neither side of the system is favored and the reaction is in equilibrium.
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Re: When Q=K
Hi,
When Q = K, the reaction is at equilibrium—and will remain so until the system is disturbed (e.g. if heat is added or the pressure is increased).
Here is a diagram that illustrates the comparison between the reaction quotient (Q) and equilibrium constant (K):
When Q = K, the reaction is at equilibrium—and will remain so until the system is disturbed (e.g. if heat is added or the pressure is increased).
Here is a diagram that illustrates the comparison between the reaction quotient (Q) and equilibrium constant (K):
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Re: When Q=K
Yep! The reaction quotient is usually measured and calculated multiple times as a reaction precedes, and when it finally equals K, it indicates that the system is at equilibrium and the reactions are occurring at the same rate.
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Re: When Q=K
Yes, if Q=K, then the reaction is at equilibrium. This will always be the case. If Q does not equal K, then it's not at equilibrium.
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Re: When Q=K
Yes, if Q is equal to K that means that the reaction is at equilibrium. If Q is any other value besides K it is not at equilibrium.
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Re: When Q=K
Yep! When the reaction quotient is the same thing as the equilibrium constant, then the reaction is at equilibrium.
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Re: When Q=K
Yes, when Q is equal to K it means that the reaction is at equilibrium. When Q is any other value, it means that the reaction is not at equilibrium. Hope this helps!
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Re: When Q=K
Yes, if the ratio of products to reactants equals K then we can say Q=K, which means the reaction is at equilibrium.
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Re: When Q=K
Yes, this is the case as K is the numerical value of Q at the "end" of the reaction when equilibrium has been reached. Hope that helps!
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Re: When Q=K
Yes! K is the ratio of the concentrations of the products and reactants at equilibrium. When the reaction quotient (the same ratio, but at any given point in time or progression of the reaction) is equal to K, the system is at equilibrium.
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Re: When Q=K
Yes, Q is basically the same as K in how it is calculated, it is just called K at equilibrium and Q when not at equilibrium. When K = Q it is at equilibrium.
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Re: When Q=K
Yes, Q and K are calculated the same way, so if Q is equal to K, the system is at equilibrium.
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Re: When Q=K
Yes, when Q=K the reaction is at equilibrium. If Q<K then we can predict the reaction will favor the products until K is reached. When the calculated Q value > K then we can predict the reactants will be favored, going right to left.
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Re: When Q=K
Yes, Q will proceed to move in the direction that gets the system to equilibrium (when Q=K).
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Re: When Q=K
If Q=K then yes this means that the reaction is at equilibrium. The reaction quotient, Q, will equal the equilibrium constant,K, meaning the reaction itself is at a balance.
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Re: When Q=K
Yes, if Q=K then the reaction must be at equilibrium. Since K is the equilibrium constant (signifying the reaction is at equilibrium), if the reaction quotient, Q, is equal to it, then the reaction has reached equilibrium.
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Re: When Q=K
Yes, when Q = K the reaction is considered to be at equilibrium. Q measures the relative product and reactant concentrations at a specific point in time, which may or may not be equal to the product and reactant concentrations at equilibrium (K).
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Re: When Q=K
Both Q and K are derived through the concentrations of products/reactants. If Q and K are equivalent that means the system is at equilibrium and the value is no longer "Q" but instead it is "K"
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Re: When Q=K
Yes, when Q is = to K, it indicates that the reaction is at equilibrium. Conversely, we know that when q is not = K, the reaction is not at equilibrium.
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Re: When Q=K
If the Q is a big number because the numerator is large, that means there are more products so it would need to shift left towards reactants. If it is a smaller number, then Q would be more reactant heavy and shift to the right toward the products.
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Re: When Q=K
Yes. You can assume that it is at equilibrium since the ratios of the concentrations are the same. Hope this helps!
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Re: When Q=K
Yes, when Q = K it is safe to assume that the reaction is at equilibrium since K is used only when the reaction is at equilibrium.
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Re: When Q=K
Yes. Since k is the constant for the reaction at equilibrium, if Q is equal to K it must mean that equilibrium has been reached.
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Re: When Q=K
When you are checking if a reaction has reached equilibrium and you compare Q to K (which would be given), and Q=K, the reaction is at equilibrium.
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Re: When Q=K
Only when the reaction quotient(Q) equals the equilibrium constant(K) will the reaction be in equilibrium.
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Re: When Q=K
Yes, when Q=K, the reaction is at equilibrium. This is because K is the ratio of product concentration over reactant concentration at equilibrium, and Q is the exact same thing but when the reaction is at an undetermined state. Therefore, when they are equal, the reaction state is determined to be equilibrium.
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Re: When Q=K
Yep. K is the equilibrium constant so if Q is the same as K, you assume the reaction is in equilibrium.
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Re: When Q=K
Yes, when Q=K the system is at equilibrium. The formulas for Q and K are the same, K just specifies the concentrations/pressures are at equilibrium.
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Re: When Q=K
Yup! if q=k, it is at equilibrium since they use the same formula, the only difference is the context in which you label them.
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Re: When Q=K
Although a very rare instance, when Q=K, it is safe to assume that the reaction is at equilibrium.
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Re: When Q=K
Yes if you have K, and solve the ratio of products over reactants and find that Q is equal to K, then you can assume that the reaction is at equilibrium.
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Re: When Q=K
Yes the reaction is at equilibrium when Q=K. This is because K is the equilibrium constant while Q is the ratio when the reaction is NOT at equilibrium therefore if Q DOES equal K, the ratio is equal to the equilibrium ratio making it at equilibrium.
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Re: When Q=K
Hi, yes when Q=K the reaction is at equilibrium. You can compare the two to see which side is favored as well. Hope this helps!
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Re: When Q=K
Yes ! this is true because if Q is the ratio of products to reactants and K is the ratio of those at equilibrium and then Q =K then we can assume the reaction is at equilibrium.
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