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which statement is not always correct for a reaction at equilibrium a the concentration of the reactants and products are equal well in fact this is the answer because they are definitely not always the same this is implying it is an exactly 50 50 equilibrium with exactly 50 reactants and products and that is in fact rarely the case so a is the correct answer B is a true statement equilibrium can be achieved starting from the reactants or in fact the product as is mentioned in part C thatamp;#39;s a characteristic of equilibrium it can be approached from either direction so B and C both true statements and D the rate of the forward reaction is equal to the rate of a reverse reaction again that is one of the definitions of a system in equilibrium and so b c and d are true statements about a closed system at equilibrium a is a false statement and so is the correct answer here
