K and Q
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Re: K and Q
If K and Q are equal that means the system is at equilibrium because the ratio of the products to reactants is the same for K and Q and therefore, the system has the correct ratio of products to reactants needed for equilibrium. Since Q is equal to K the reaction will not favor one direction but will proceed at equal rates in both directions.
Re: K and Q
Yes, because when Q is equal to K the ratio of products to the reactants at the moment in question is the concentrations for the equilibrium of that reaction.
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Re: K and Q
Additionally, if K and Q aren't equal, you know the equation is not in equilibrium. So If Q < K at some time during reaction, then [R] > [P] and the forward reaction is favored. If Q > K at some time during reaction, then [P] > [R] and the reverse reaction is favored.
Re: K and Q
Yes, because the equation used to find both are the exact same. The K value is when the reaction is at equilibrium so if Q equates to that then the reaction is definitely at equilibrium as well.
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Re: K and Q
Yes. If Q>K, then the reaction will create more reactants and if Q<K, the reaction will create more products.
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