This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Let's solve this! Step 1: Write the balanced chemical equation for the reaction. Iron reacts with copper(II) sulfate solution in a single displacement reaction: Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s) The equation is already balanced, showing a 1:1 mole ratio between iron (Fe) and copper (Cu). Step 2: Calculate the number of moles of iron (Fe). We'll use the molar mass of iron (Fe ≈ 55.845 g/mol). Moles of Fe = mass / molar mass Moles of Fe = (28 g) / (55.845 g/mol) Moles of Fe ≈ 0.5014 mol Step 3: Determine the number of moles of copper (Cu) deposited. From the balanced equation, 1 mole of Fe reacts to produce 1 mole of Cu. Therefore, moles of Cu = moles of Fe Moles of Cu ≈ 0.5014 mol Step 4: Calculate the mass of copper (Cu) deposited. We'll use the molar mass of copper (Cu ≈ 63.546 g/mol). Mass of Cu = moles × molar mass Mass of Cu = (0.5014 mol) × (63.546 g/mol) Mass of Cu ≈ 31.86 g Rounding to two significant figures (based on the given 28g), the mass of copper deposited is 32 g. The amount of copper deposited will be 32 g. Send me the next one 📸