\[ 2 \mathrm{Ag}+\mathrm{H}_{2} \mathrm{~S} \rightarrow \mathrm{Ag}_{2} \mathrm{~S}+\mathrm{H}_{2} \] According to the equation for this chemical reaction, what does the \( \mathbf{2} \) in front of 2 Ag tell us? A Two atoms of silver are lost in this reaction. B Two atoms of silver are produced by this reaction. C Two atoms of silver are needed to complete the reaction. D Two atoms of silver are gained to produce silver sulfide.

The \( \mathbf{2} \) in front of \( 2 \mathrm{Ag} \) indicates that two atoms of silver are needed to complete the reaction. So, the correct answer is C. This tells us that for every reaction of hydrogen sulfide with silver, we need two silver atoms to form the product, silver sulfide. Additionally, silver sulfide (\( \mathrm{Ag}_2\mathrm{S} \)) is a fascinating compound often found in tarnished silverware. Its formation is a result of silver reacting with sulfur compounds in the air, leading to that distinctive black tarnish. Cleaning your silver is not just about aesthetics but also about halting this reaction! Also, did you know that silver sulfide has applications beyond just being an unsightly tarnish? In mineralogy, it is sought for its properties and is intriguing in studies related to semiconductor behavior. So, silver isn’t just shiny; it's got some hidden talents too!