Q and K
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Re: Q and K
Q is the reaction quotient and K is the equilibrium. Q basically tells us the ratio of the concentration or partial pressure of the products to that of the reactants when the reaction is not at equilibrium, while K tells the same thing when the reaction is at equilibrium. Comparing the two not only tells us whether or not the reaction is at equilibrium but can also tell us what direction the reaction will proceed in to reach equilibrium if it is not already at equilibrium. If QK then the reverse reaction will be favored. If QK then the forward reaction will be favored.
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Re: Q and K
K tells us the equilibrium constant and Q is the ratio of the concentration of products and reactants at any given time. You can use K to find whether a reaction is in equilibrium and which side it it more likely to favor. If Q is less than K then the reaction will shift right and if Q is greater then K it will shift to the right.
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Re: Q and K
K uses only equilibrium concentrations. Q can use any concentration at any time, which tells us where the reaction will go.
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Re: Q and K
K is the equilibrium constant so the reaction needs to be at equilibrium in order for us to calculate K. Q, on the other hand, can be calculated at any time during the reaction and there does not need to be an equilibrium.
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Re: Q and K
If Q < K, then [R] > [P] and forward reaction is favored
If Q > K, then [R] < [P] and reverse reaction is favored
Q=K then reaction is at equilibrium
If Q > K, then [R] < [P] and reverse reaction is favored
Q=K then reaction is at equilibrium
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Re: Q and K
Q and K are very similar, at equilibrium Q = K but any other time than that Q won't equal K but it will tell us which side will be favored in order to get to K.
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Re: Q and K
The value Q is useful because in comparison to a K value for a reaction it tells us whether products or reactants are favored (which direction the reaction will go towards)
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Re: Q and K
If Q > K then a reverse reaction is favored.
If Q < K then a forward reaction is favored.
If Q < K then a forward reaction is favored.
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Re: Q and K
Q is the reaction quotient which can be at any time.
K is the equilibrium constant (only at equilibrium, duh.)
If Q > K then the reverse reaction is favoured.
If Q < K then the forward reaction is favoured.
Basically, it tells us which direction the reaction sits.
K is the equilibrium constant (only at equilibrium, duh.)
If Q > K then the reverse reaction is favoured.
If Q < K then the forward reaction is favoured.
Basically, it tells us which direction the reaction sits.
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