Question 1: Define a carbonate ion and give an example of a common carbonate compound.

Answer: A carbonate ion (CO3^2-) is a polyatomic ion consisting of one carbon atom bonded to three oxygen atoms; an example is calcium carbonate (CaCO3).

Question 2: Explain the chemical reaction that occurs when a carbonate reacts with an acid, including the key products formed.

Answer: When a carbonate reacts with an acid, it produces carbon dioxide gas, water, and a salt. The general reaction is: carbonate + acid → salt + CO2 + H2O.

Question 3: Describe how the reaction of carbonates with acids can be used to test for the presence of carbonate ions in a sample.

Answer: Adding acid to the sample and observing the production of bubbles (carbon dioxide) indicates the presence of carbonate ions.

Question 1: Calculate the volume of carbon dioxide (CO2) at room temperature and pressure produced when 5.00 g of calcium carbonate (CaCO3) reacts completely with excess hydrochloric acid. (Molar mass of CaCO3 = 100.09 g/mol, molar volume of gas = 24 dm³/mol).

Answer: V = (n × 24 dm³/mol) = [(5.00 g / 100.09 g/mol) × 24 dm³/mol] ≈ 1.20 dm³.

Question 1: Design a simple experiment to test whether a sample of rock contains carbonate minerals. Mention the key variables and safety precautions you would take.

Answer: To test for carbonate minerals, place a small piece of the rock in a test tube, add dilute hydrochloric acid, and observe for bubbles of CO2. Key variables include acid concentration and sample size. Safety precautions include wearing goggles and gloves, and working in a well-ventilated area to avoid inhaling gases.

Question 1: A renewable energy company uses carbonate-based materials to capture CO2 emissions. They report that 250 g of carbonate reacts completely to produce 60 dm³ of CO2 at room temperature and pressure. Does this data align with the molar calculations? Show your reasoning.

Answer: Calculations show that 250 g of CaCO3 (molar mass 100.09 g/mol) produces about 2.5 mol, which should generate 2.5 mol × 24 dm³/mol = 60 dm³ of CO2, confirming the data aligns with theoretical expectations.

Question 1: Explain how the reaction of carbonates with acids can be utilised to capture and store carbon dioxide in renewable energy systems.

Answer: Carbonates react with acids to produce CO2, which can be captured and stored in renewable energy processes such as mineral carbonation, helping to reduce greenhouse gas emissions.

Question 2: Discuss the advantages and limitations of using carbonate-based materials for CO2 capture in renewable energy applications.

Answer: Advantages include the abundance and stability of carbonate minerals, and their potential for permanent CO2 storage. Limitations involve the energy-intensive processes required for mineral carbonation, slow reaction rates, and challenges in scaling up for industrial use.