Question

Use the pull-down menus to specify the state of each reactant and product. Ag2S 2Ag + S2- Is silver sulfide considered soluble or not soluble ? ... ... A. Soluble ... B. Not soluble Based upon this, the equilibrium constant for this reaction will be: ... ... A. Greater than 1 ... B. Less than 1 Submit AnswerRetry Entire Group

Answer 1

Step-by-step explanation:

For the given reaction equation, we will write the state of each specie as follows.

`Ag_(2)S(s) \rightarrow 2Ag^(+)(aq) + S^(2-)(aq)`

Since, silver sulfide (
`Ag_(2)S`) will remain in solid state. Therefore, it acts as a precipitate, that is, insoluble solid. Hence, it is insoluble.

And, expression for the equilibrium constant of this reaction is as follows.

`K_(eq) = ([Ag^(+)]^(2)[S^(2-)])/([AgS]^(2))`

For solids, it is considered to be equal to 1. Hence, the equilibrium constant expression will be as follows.

`K_(eq) = [Ag^(+)]^(2)[S^(2-)]`

Therefore, we can conclude that its equilibrium constant for this reaction will be greater than 1.