Question

In a reaction between copper metal and an aqueous iron (III) chloride, Fe₃⁺(aq) is reduced to Fe₂⁺(aq), while Cu(s) is oxidized to Cu₂⁺(aq). Determine the mass of Cu(s) required to react with 26.9 ml of 1.9 M FeCl₃(aq).

Answer 1

To determine the mass of copper (Cu) required to react with a given volume and molarity of FeCl₃, one must convert volume to moles, use stoichiometry to find moles of copper needed,

Step-by-step explanation:

The student has asked about the mass of copper (Cu) required to react with a certain volume and molarity of aqueous iron (III) chloride (FeCl₃). To answer this question, we first need to convert the volume of FeCl₃ to moles using its concentration. Then, we use stoichiometry to determine the moles of copper required for the reaction and finally convert this amount to grams.

To start, we calculate the moles of FeCl₃: 1.9 mol/L * 0.0269 L = 0.05111 mol FeCl₃. In this redox reaction, three moles of copper react with two moles of Fe₃⁺⁻ ions (as obtained from the balanced chemical equation), so we can calculate the moles of Cu required: (3 moles Cu / 2 moles Fe₃⁺⁻) * 0.05111 mol FeCl₃ = 0.076665 mol Cu.

Now, knowing the molar mass of copper is approximately 63.55 g/mol, we can find the mass of copper:
0.076665 mol Cu * 63.55 g/mol = 4.8730 g of Cu.

The answer is that 4.8730 grams of copper are required to react with 26.9 mL of 1.9 M FeCl₃ solution.