Q vs K [ENDORSED]
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Re: Q vs K
K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage of a reaction. The direction of a reaction can be determined by comparing Q and K.
The difference is that equilibrium constant (K) is the ratio between the concentrations of products and the concentrations of reactants at equilibrium.
The difference is that equilibrium constant (K) is the ratio between the concentrations of products and the concentrations of reactants at equilibrium.
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Re: Q vs K
As mentioned above, K as the equilibrium constant is calculated when the reaction is in equilibrium. Q, the reaction quotient, is found when the reaction is at any point other than equilibrium- in other words, when the reaction is not at equilibrium. While K and Q are calculated the same way ([P]/[R]), comparing the two values is helpful in indicating which direction a reaction will proceed. For instance, when Q > K, more products/insufficient reactants are present at that instance than during equilibrium, so the reaction will proceed towards the left to make more reactants.
Re: Q vs K [ENDORSED]
Q can be calculated at any given point of the reaction. K is calculated when the system is in equilibrium.
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Re: Q vs K
The Q is the same thing as the K value however it is the constant when the reaction is not in equilibrium. So you often compare K and Q to see which side of the reaction is favored when it is not in equilibrium.
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