Question 1: Aqueous electrolysis involves passing an electric current through an aqueous solution to decompose it into its constituent elements. This process can produce gases or elements at the electrodes. Explain in your own words what happens during aqueous electrolysis.

Answer: During aqueous electrolysis, an electric current passes through an aqueous solution, causing ions to move toward electrodes where they are reduced or oxidized, resulting in the formation of new substances such as gases or elements at the electrodes.

Question 1: Define electrolysis and describe the role of electrodes in this process.

Answer: Electrolysis is a chemical process where an electric current decomposes a compound into its elements. Electrodes are conductors through which the current enters and leaves the solution, allowing ions to be reduced or oxidized.

Question 2: In aqueous electrolysis of sodium chloride solution, what gases are typically formed at the anode and cathode?

Answer: Chlorine gas at the anode and hydrogen gas at the cathode.

Question 1: During electrolysis of water, 96,000 coulombs of charge are passed through the water. How many moles of hydrogen gas are produced? (Use Faraday's constant: 96485 C/mol).

Answer: 0.5 mol

Question 2: Calculate the volume of hydrogen gas produced at room temperature and pressure when 2 moles of hydrogen are generated during electrolysis. (Use 22.4 L/mol for molar volume).

Answer: 44.8 L

Question 1: List three safety precautions to consider when setting up an electrolysis experiment in the laboratory.

Answer: Wear safety goggles, avoid touching electrodes during operation, and ensure proper ventilation to avoid gas accumulation.

Question 2: Identify three variables that can affect the products formed during aqueous electrolysis and explain how they influence the outcome.

Answer: Variables include the type of solution (which determines the ions available), the voltage applied (which influences which ions are reduced or oxidized), and electrode material (which can catalyze or inhibit certain reactions).

Question 1: In an electrolysis experiment of dilute sulfuric acid, hydrogen gas is collected at the cathode, and oxygen gas at the anode. If 2.0 liters of hydrogen are collected, what volume of oxygen is expected? (Assume gases are at the same conditions of temperature and pressure).

Answer: 1.0 liter

Question 1: Describe one industrial application of aqueous electrolysis and explain its importance.

Answer: Electrolysis is used in the production of aluminum metal from bauxite ore, which is important for manufacturing aircraft, packaging, and construction materials.

Question 2: How might advances in electrolysis technology contribute to sustainable energy solutions?

Answer: Advances in electrolysis can improve the efficiency of producing hydrogen fuel from water, offering a clean energy source that reduces reliance on fossil fuels and helps reduce greenhouse gas emissions.