Relationship between K and G
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Relationship between K and G
If Q<K does this imply that delta G is negative, meaning that it will progress in the forward direction or must be still consider temperature, enthalpy, and entropy values as well?
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Re: Relationship between K and G
I believe you're right.
If (Q/K) <1 or Q < K, then delta G will be negative and thus spontaneous reaction.
If (Q/K) >1 or Q > K, then delta G will be positive and thus non-spontaneous reaction.
Hope this helps!
If (Q/K) <1 or Q < K, then delta G will be negative and thus spontaneous reaction.
If (Q/K) >1 or Q > K, then delta G will be positive and thus non-spontaneous reaction.
Hope this helps!
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Re: Relationship between K and G
It helps to think of this in terms of k in an equilibrium equation to determine whether it will proceed to reactants vs products.
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Re: Relationship between K and G
if Q<K and it's spontaneous does that mean the forward reaction is stable?
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