Which of the following statements is true about a reversible reaction?
all reversible reactions have low activation energy
when we mix the reactants together one or more of the reactants will be completely used up
when we mix the reactants together none of the reactants will be completely used up
Answer:
Technically, I think it's none of the above.
The question says nothing about the amount of heat or energy put into the reaction, so statements about exothermicity or activation energy are kind of irrelevant. If you put enough energy in, most reactions are going to be reversible; it ends up being an equilibrium between reactants and products. The only possible choice would be D, that none of the reactants will be completely used up. This is technically not true, because again, it's an equilibrium issue. All reversible reactions exist in an equilibrium between reactants and products. If the reaction is pushed far enough toward the product, you could technically have a reversible reaction where all of the reactants are consumed. So while I think that technically the answer is none of the above, if you feel like you have to choose one of them, it's definitely D.
Good luck!
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