the equilibrium constant, K, is greater than one. The stronger acid in this system is and the weaker base is .

The question is incomplete; the complete question is;

For the following reaction:

H2CO3 + S2- > HCO3- + HS-

The equilibrium constant is greater than one. The strongest acid in this system is and the weakest base is .

A) H2CO3 and HS-                  

B) S2- and HS-                        

C) HCO3- and S2-                    

D) HS- and S2-

E) H2CO3 and HCO3-

H2CO3 and HS-  

Explanation:

According to the Brownstead- Lowry theory of acids and bases, an acid is a proton donor while a base is specie that accepts protons.

A strong acid has a greater tendency to donate protons. If we look at the reaction, H2CO3 has the greatest ability to donate protons hence it is the strongest acid.

On the other hand, HS- has the least ability to accept protons so it is the weakest base.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.

answer would be option a) they have mobile charged particles.