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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? 2(108 g/mol)+32 g/mol=248 g/mol; (248 g/mol)(0.04 mol)=9.92  108 g/mol+2(32 g/mol)=172 g/mol; (172 g/mol)(0.02 mol)=3.44 g

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? 2(108 g/mol)+32 g/mol=248 g/mol; (248 g/mol)(0.04 mol)=9.92  108 g/mol+2(32 g/mol)=172 g/mol; (172 g/mol)(0.02 mol)=3.44 g

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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?

  • 2(108 g/mol)+32 g/mol=248 g/mol; (248 g/mol)(0.04 mol)=9.92 
  • 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)(0.04 mol)=6.88 g
  • 2(108 g/mol)+32 g/mol=248 g/mol; (248 g/mol)(0.02 mol)=4.96 g
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