Respuesta :

Edufirst

Answer:

        [tex]\large\boxed{\large\boxed{3.894g}}[/tex]

Explanation:

From similar question, equation (b) is

Molecular Equation:

  • Cu(s) + 2AgNO₃(aq) → Cu(NO₃)₂(aq) + 2Ag(s)

Net Ionic Equation:

  • Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)

1. Mole ratio:

       [tex]\dfrac{2molAg(s)}{1molCu(s)}[/tex]

2. Convert 1.147 g of Cu(s) to moles:

  • Atomic mass of Cu: 63.546g/mol

  • Number of moles = mass in grams / atomic mass

  • Number of moles = 1.147 g / 63.546 g/mol = 0.01805 mol Cu(s)

3. Calculate the moles of Ag(s):

    [tex]0.01805molCu(s)\times \dfrac{2molAg(s)}{1molCu(s)}=0.03610molAg(s)[/tex]

4. Convert 0.03610 mol Ag(s) to grams:

  • Atomic mass of Ag(s) = 107.868g/mol

  • Mass = 0.03610mol × 107.868g/mol = 3.894g

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