Electrolysis of a CuSO4 produces

To answer the question step by step, we need to understand the process of electrolysis and how it relates to the compound CuSO4.

Step 1: Understanding Electrolysis Electrolysis is a chemical process that uses an electric current to drive a non-spontaneous chemical reaction. It involves the decomposition of an electrolyte, which is a substance that conducts electricity when dissolved in a solvent.

Step 2: Understanding CuSO4 CuSO4 is the chemical formula for copper(II) sulfate. It is an electrolyte that can conduct electricity when dissolved in water. In its dissolved form, it dissociates into copper ions (Cu2+) and sulfate ions (SO4^2-).

Step 3: Electrolysis of CuSO4 When CuSO4 is subjected to electrolysis, the copper ions (Cu2+) and sulfate ions (SO4^2-) will migrate towards the electrodes due to the electric current.

Step 4: Electrodes Electrodes are conductive materials that are used to facilitate the flow of electric current during electrolysis. There are two types of electrodes: the anode and the cathode.

Step 5: Anode The anode is the positive electrode. During electrolysis of CuSO4, the copper ions (Cu2+) will be attracted to the anode. At the anode, oxidation occurs, and copper ions lose electrons to form copper atoms.

Step 6: Cathode The cathode is the negative electrode. During electrolysis of CuSO4, the sulfate ions (SO4^2-) will be attracted to the cathode. At the cathode, reduction occurs, and water molecules gain electrons to form hydrogen gas (H2) and hydroxide ions (OH^-).

Step 7: Overall Reaction The overall reaction during electrolysis of CuSO4 can be summarized as follows: At the anode: Cu2+ + 2e- -> Cu At the cathode: 2H2O + 2e- -> H2 + 2OH^- Overall: Cu2+ + 2H2O -> Cu + H2 + 2OH^-

In conclusion, electrolysis of CuSO4 produces copper metal (Cu) at the anode and hydrogen gas (H2) and hydroxide ions (OH^-) at the cathode.