1.703 g Copper
We can begin by writing the balanced equation for the reaction;
Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s)
We are given;
Mass of Zn = 1.75 g
Volume of CuSO₄ = 50 mL
Molarity of CuSO₄ = 0.75 M
Required to identify the metal formed and its mass
Moles of Zn
Moles = Mass ÷ Molar mass
Molar mass of Zn = 65.38 g/mol
Moles of Zn = 1.75 g ÷ 65.38 g/mol
= 0.0268 moles
Moles of CuSO₄
Moles = Molarity × Volume
Moles of CuSO₄ = 0.75 M × 0.050 L
= 0.0375 moles
Since, from the reaction 1 mole of Zn reacts with 1 mole of CuSO₄
Then, Zn is the rate limiting reaction since it has less number of moles available.
1 mole of Zn reacts to form 1 mole of Cu
Thus, number of moles of Zn will be equal to the number of moles of Cu
Hence, moles of copper = 0.0268 mole
Mass = Moles × Molar mass
Molar mass of Copper = 63.546 g/mol
Therefore;
Mass of Copper = 0.0268 moles × 63.546 g/mol
= 1.703 g
Therefore, the metal formed is copper with a mass of 1.703 g
