In a chemical reaction, dynamic equilibrium occurs when the rate of the forward reaction becomes precisely equal to the rate of the reverse reaction. All of the following statements are true EXCEPT:
A. A dynamic equilibrium occurs when the reaction is more than 50 percent complete.
B. In a dynamic equilibrium, reactants are converted to products at the same rate as products become reactants.
C. Reactions that reach a dynamic equilibrium are often referred to as reversible reactions.
D. Reactions that reach a dynamic equilibrium are shown with a double arrow, to indicate the forward and reverse reactions.
E. Reactions that reach equilibrium very close to the end (product side) are usually shown with only one arrow instead of a double arrow, and we say the reaction goes to completion.
Answer (2)
Nope. The definition talks about the RATES in each direction, but there's no reason that it must happen at any particular STAGE during the whole thing. Choice 'E' even talks about a reaction that doesn't reach equilibrium until it's almost done. The one you want is 'A'.
The statement that is not true is A: 'A dynamic equilibrium occurs when the reaction is more than 50 percent complete.' because dynamic equilibrium can occur at any point, not just when a reaction is significantly complete.
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