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?

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?

108 g/mol+2(32 g/mol)=172 g/mol; (172 g/mol)(0.04 mol)=6.88 g
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)(1mol Ag2S / 2mol Ag) =4.96 g
108 g/mol+2(32 g/mol)=172 g/mol; (172 g/mol)(0.04 mol)(1mol Ag2S / 2molAg)=3.44 g

Answer 1

The correct steps to determine the mass of silver sulfide (Ag2S) produced in the reaction are:

1) Calculate the molar mass of Ag2S:
108 g/mol + 2(32 g/mol) = 172 g/mol

2) Multiply the molar mass of Ag2S by the number of moles of silver (Ag) used in the reaction:
(172 g/mol)(0.04 mol) = 6.88 g

Therefore, the correct answer is:
(172 g/mol)(0.04 mol) = 6.88 g