If an excess of zinc metal is placed in a copper(I) sulfate solution, the zinc will displace the copper.
If 10.8 g of copper(lI) sulfate is reacted, how many grams of copper metal will be recovered from the solution? (Hint: Za + CuSO, → 2nSO, + Cu.)
First, we need to determine the molar mass of CuSO4:
Cu: 63.55 g/mol
S: 32.07 g/mol
O: 16.00 g/mol
Total molar mass = 63.55 + 32.07 + (4 x 16.00) = 159.73 g/mol
Next, we need to determine the number of moles of CuSO4:
10.8 g / 159.73 g/mol = 0.0676 mol
From the balanced chemical equation, we can see that 1 mole of CuSO4 produces 1 mole of Cu. Therefore, the number of moles of Cu produced will also be 0.0676 mol.
Now, we can calculate the mass of Cu recovered:
Mass = number of moles x molar mass
Mass = 0.0676 mol x 63.55 g/mol = 4.30 g
Therefore, 4.30 grams of copper metal will be recovered from the solution.