Q vs K
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Re: Q vs K
K is the ratio of products to reactants at equilibrium, while Q is the ratio of products to reactants at any given point in the reaction (not necessarily equilibrium).
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Re: Q vs K
K is the constant you get for the ratio of the concentration of products at equilibrium to the concentration of reactants at equilibrium. Q is the ratio of products to reactants at any time. Q is used as a point of comparison to K to determine which direction the reaction will proceed to reach equilibrium.
Last edited by Ally Huang- 1F on Thu Jan 09, 2020 3:23 pm, edited 1 time in total.
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Re: Q vs K
K is the ratio of products over reactants at equilibrium, Q is the same thing not at equilibrium
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Re: Q vs K
Q is used when the reaction is not at equilibrium and K is the ratio of products to reactant when the system is at equilibrium.
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Re: Q vs K
Q and K are calculated the same but Q is the value at any point during the reaction while K is the value at equilibrium.
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Re: Q vs K
If Q is less than K at some time during the reaction, then compared to the equilibrium concentrations [R] > [P] and the forward reaction is favored, and vice versa.
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Re: Q vs K
Q is used to evaluate the concentration of reactants and products at any given point in a reaction. If Q = K, then the reaction is in equilibrium at that time. If Q>K, then that means there are more reactants present at that time than there would be if the reaction was in equilibrium. If Q<K, that means that there are more products at that point than there would be if the reaction was in equilibrium.
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