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
Hey Joy, good to see you again. Step 1: Write the half-reaction for the deposition of copper. Copper (II) ions gain electrons to form solid copper. Cu^2+(aq) + 2e^- Cu(s) This reaction shows that 2 moles of electrons are required to deposit 1 mole of copper. Step 2: Calculate the number of moles of copper deposited. Given mass of copper = 24 g Molar mass of copper (Cu) = 64 g/mol Moles of Cu = Mass of CuMolar mass of Cu Moles of Cu = 24 g64 g/mol Moles of Cu = 0.375 mol Step 3: Calculate the number of copper atoms deposited. Avogadro's number (N_A) = 6.022 × 10^23 atoms/mol Number of Cu atoms = Moles of Cu × N_A Number of Cu atoms = 0.375 mol × 6.022 × 10^23 atoms/mol Number of Cu atoms = 2.25825 × 10^23 atoms Step 4: Calculate the total number of electrons. From Step 1, 1 atom of Cu requires 2 electrons. Total number of electrons = Number of Cu atoms × 2 Total number of electrons = 2.25825 × 10^23 × 2 Total number of electrons = 4.5165 × 10^23 The number of electrons present is 4.5165 × 10^23. Send me the next one 📸