$$ 2 \mathrm{Ag}+\mathrm{H}_{2} \mathrm{~S} \rightarrow \mathrm{Ag}_{2} \mathrm{~S}+\mathrm{H}_{2} $$ 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.

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UpStudy AI · Accepted Answer

In the given chemical reaction:

$$
2 \mathrm{Ag} + \mathrm{H}_{2} \mathrm{~S} \rightarrow \mathrm{Ag}_{2} \mathrm{~S} + \mathrm{H}_{2}
$$

the coefficient $$ \mathbf{2} $$ in front of $$ \mathrm{Ag} $$ indicates the number of silver (Ag) atoms required for the reaction. Specifically, it means that **two atoms of silver are needed** to react with one molecule of hydrogen sulfide ($$ \mathrm{H}_{2}\mathrm{S} $$) to form one molecule of silver sulfide ($$ \mathrm{Ag}_{2}\mathrm{S} $$) and one molecule of hydrogen gas ($$ \mathrm{H}_{2} $$).

**Correct Answer:**  
C Two atoms of silver are needed to complete the reaction.
The $$ 2 $$ in front of $$ \mathrm{Ag} $$ means two atoms of silver are needed to complete the reaction.

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