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So in the context of equilibrium from 14A and the context of this chapter how does the values of K and Q in reference to their value against 1 (If K is greater than 1, then x. If K is less than 1, then y). Are the concepts the same no matter the contexts? Or do they change depending on which chapter's context we are applying.
These concepts are overarching within chemistry. If K is much larger than 1, then the reaction heavily favors the products(as written). If Q>K, then more reactants will be formed. Similarly, if Q<K then more product will be formed.
The concepts remain true throughout chemistry, but it is true that there may be additional methods such as Gibbs Free Energy that we may learn to determine if a reaction is at equilibrium and in which direction it will occur if it is not.
The concepts of Q and K are the same the variable changes depending on the context of the question. Q is used when referring to two concentrations that are not at equilibrium and can be utilizded at any point of the reaction. Whereas K is used when referring to concentrations at equilibrium. Q can be compared to K when determining which way the reaction is favoring. I believe if Q> K the reaction favors the reactants and if Q<K the reaction favors the products. If Q=K then the reaction is at equilibrium because the ratio is the same.
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