Question

What mass of metallic silver can form from 1.147 g of copper metal according to equation b?

Answer 1

Answer:

        $\large\boxed{\large\boxed{3.894g}}$

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:

       $\dfrac{2molAg(s)}{1molCu(s)}$

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):

    $0.01805molCu(s)\times \dfrac{2molAg(s)}{1molCu(s)}=0.03610molAg(s)$

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