Chemical Reaction Overview
📌 The experiment involves reacting copper(II) sulfate ($\text{CuSO}_4$) solution with iron metal ($\text{Fe}$) to produce pure copper ($\text{Cu}$) and iron sulfate ($\text{FeSO}_4$ or $\text{Fe}_2(\text{SO}_4)_3$).
🧪 7 grams of anhydrous copper(II) sulfate were dissolved in heated water; the anhydrous form is noted to be almost white.
⚡ Agitation or stirring speeds up the reaction rate by increasing the frequency of atomic and molecular collisions.

Reaction Observation and Separation
💧 After the reaction, the copper product settled at the bottom, leaving a blue solution behind, indicating the consumption of $\text{Cu}^{2+}$ ions.
⚖️ The initial mass of the filter paper used for separation was 1.50 g.
✨ The wet copper product, trapped in the filter paper, was rinsed with distilled water to maximize product recovery for a higher percent yield.

Product Yield Determination
☀️ The product (copper in filter paper) was allowed to dry overnight in the fume hood for accurate weighing.
⚖️ The final mass of the copper product plus the filter paper was 3.96 g.
📊 The mass of the pure copper product is calculated by subtracting the filter paper mass from the final mass ($3.96 \text{ g} - 1.50 \text{ g}$).

Key Points & Insights
➡️ To ensure maximum product isolation, use distilled water to rinse all residual product from the reaction beaker onto the filter paper.
➡️ The color of the leftover solution after filtration provides a crucial clue for determining the limiting and excess reagents.
➡️ Reaction speed is directly proportional to the frequency of molecular collisions achieved through methods like stirring.

📸 Video summarized with SummaryTube.com on Nov 20, 2025, 05:29 UTC