Question

Use the chemical equation to answer the question.

2Ag(s) + H2S(g) → Ag2S(s) + H2(g)

The molar mass of silver (Ag) is 108 g/mol. The molar mass of sulfur (S) is 32 g/mol. The reaction uses 0.04 mol of silver. Which steps show how to determine the mass of silver sulfide (Ag2S) produced in the reaction?

(1 point)
Responses

2(108 g/mol)+32 g/mol=248 g/mol
; (248 g/mol)(0.04 mol)=9.92 g

2(108 g/mol)+32 g/mol=248 g/mol
; (248 g/mol)(0.04 mol)=9.92 g


108 g/mol+2(32 g/mol)=172 g/mol
; (172 g/mol)(0.02 mol)=3.44 g

108 g/mol+2(32 g/mol)=172 g/mol
; (172 g/mol)(0.02 mol)=3.44 g


2(108 g/mol)+32 g/mol=248 g/mol
; (248 g/mol)(0.02 mol)=4.96 g

2(108 g/mol)+32 g/mol=248 g/mol
; (248 g/mol)(0.02 mol)=4.96 g


108 g/mol+2(32 g/mol)=172 g/mol
; (172 g/mol)(0.04 mol)=6.88 g

Answer 1

Correct steps:

- 2(108 g/mol) + 32 g/mol = 248 g/mol (molar mass of Ag2S)
- 0.04 mol Ag × (1 mol Ag2S / 2 mol Ag) = 0.02 mol Ag2S
- (248 g/mol)(0.02 mol) = 4.96 g Ag2S

So choose the option: "2(108 g/mol)+32 g/mol=248 g/mol ; (248 g/mol)(0.02 mol)=4.96 g."