Final answer:
To find the required mass of zinc to react with 500 ml of 1.2 M CuSO4, we calculate the moles of CuSO4 and use the stoichiometry from the balanced reaction to determine the corresponding moles of zinc needed. Then, we use the molar mass of zinc to calculate the mass required, which is 39.24 g.
Step-by-step explanation:
To determine the mass of zinc metal needed to completely react with 500 ml of 1.2 M CuSO4, we need to know the balanced chemical equation for the reaction. Assuming the reaction is as follows:
Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)
Now let's calculate the moles of CuSO4:
- 500 ml = 0.5 L
- Molarity (M) = moles of solute / liters of solution
- Moles of CuSO4 = Molarity × Volume in Liters
- Moles of CuSO4 = 1.2 M × 0.5 L = 0.6 moles
From the balanced equation, the mole ratio of CuSO4 to Zn is 1:1, so we will also need 0.6 moles of Zn.
To find the mass of Zn required:
- Molar mass of Zn = 65.4 g/mol
- Mass = moles × molar mass
- Mass of Zn = 0.6 moles × 65.4 g/mol = 39.24 g
The answer is not exactly matching any of the options provided (A, B, C, D), thus one must check for any typographical error in the options or a misunderstanding in the calculation.