Question

Pb(SO₄) 2+2Zn→2ZnSO⁴ +Pb If 0.417 mol of zinc reacts with excess lead(IV) sulfate, how many grams of zinc sulfate will be produced in the reaction?

a) 25.16 g
b) 50.32 g
c) 75.48 g
d) 100.64 g

Answer 1

Using stoichiometry, 0.417 moles of zinc produce 0.417 moles of zinc sulfate, with a molar mass of 161.45 g/mol. The calculated mass is 67.34 g, which does not match any of the answer choices, indicating a possible error.

Step-by-step explanation:

To determine the mass of zinc sulfate produced when 0.417 mol of zinc reacts with excess lead(IV) sulfate, we use stoichiometry based on the balanced chemical equation:

Pb(SO₄)2 + 2Zn → 2ZnSO4 + Pb

According to the equation, 2 moles of zinc react to produce 2 moles of zinc sulfate. Therefore, 0.417 moles of zinc will produce 0.417 moles of zinc sulfate. Next, we calculate the mass:

Molar mass of ZnSO4 = 65.38 (Zn) + 32.07 (S) + 4 × 16.00 (O) = 161.45 g/mol

Mass of ZnSO4 = 0.417 mol × 161.45 g/mol = 67.34 g

However, this mass is not one of the answer choices. It is possible there was a mistake in the question statement or answer choices provided. The mass should be recalculated or the inputs checked for accuracy.