What must be true if the forward reaction is occurring more rapidly than the reverse reaction?
What must be true if the forward reaction is occurring more rapidly than the reverse reaction?
The reaction is not reversible.
Q<K
Q=K
There are no products present.
Homework Answers
Answer is: Q < K
Because, forward reaction is faster than reverse reaction it means products are lower than the reactants...So Q gives the idea at any time which is [product]/[Reactants]. It means lower than K which is same ratio but at equilibrium.
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What must be true if the forward reaction is occurring more rapidly than the reverse reaction?
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