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

108 g/mol+2(32 g/mol)=172 g/mol


2(108 g/mol)+32 g/mol=248 g/mol


108 g/mol+2(32 g/mol)=172 g/mol


2(108 g/mol)+32 g/mol=248 g/mol

Answer 1

First find moles of Ag2S: 0.04 mol Ag × (1 mol Ag2S / 2 mol Ag) = 0.02 mol Ag2S.

Molar mass of Ag2S = 2(108 g/mol) + 32 g/mol = 248 g/mol. (The correct steps are the ones giving 248 g/mol — options 2 and 4.)

Mass = 0.02 mol × 248 g/mol = 4.96 g Ag2S.