Question

1. based on the following balanced equation,

fe (s) + cuso₄(aq) → feso₄(aq) + cu (s)
a. what is the charge on the iron in the product feso₄?
b. if 0.5206 g of iron is reacted, how many moles of copper should be produced?

Explanation:

Step1: Find Fe charge in FeSO₄

Sulfate ion ($\text{SO}_4^{2-}$) has charge -2. Let Fe charge = $x$. For neutral compound:
$$x + (-2) = 0$$
$$x = +2$$

Step2: Calculate moles of Fe

Molar mass of Fe = 55.85 g/mol. Moles = mass/molar mass:
$$n(\text{Fe}) = \frac{0.5206\ \text{g}}{55.85\ \text{g/mol}} \approx 0.009321\ \text{mol}$$

Step3: Relate moles of Fe to Cu

From balanced equation, mole ratio $\text{Fe}:\text{Cu} = 1:1$. So:
$$n(\text{Cu}) = n(\text{Fe}) = 0.009321\ \text{mol}$$

Answer:

a. +2 (or 2+)
b. 0.009321 mol