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Here are the solutions to the chemistry questions: Item one: a) Understand the nature of substance X. Step 1: Identify element X based on its atomic number and mass number. The atomic number of X is 12, and its mass number is 24. This identifies element X as Magnesium (Mg). Magnesium is an alkaline earth metal. It is a solid at room temperature and is known to burn in air, producing a bright white light. b) Determine the formula of the oxide X. Step 1: Calculate the mass of oxygen that reacted. Mass of oxygen = Mass of oxide - Mass of X Mass of oxygen = 0.5 g - 0.3 g = 0.2 g Step 2: Calculate the number of moles for Magnesium (X) and Oxygen. The molar mass of Mg is 24 g/mol, and the molar mass of O is 16 g/mol. Moles of Mg = 0.3 g24 g/mol = 0.0125 mol Moles of O = 0.2 g16 g/mol = 0.0125 mol Step 3: Determine the simplest whole number ratio of moles to find the empirical formula. Ratio of moles Mg:O = 0.0125 : 0.0125 = 1:1 The formula of the oxide is MgO. c) Know the environmental consequences of the element. The environmental consequences of magnesium primarily stem from its extraction and processing. Mining magnesium can lead to habitat destruction, soil erosion, and water pollution. Magnesium oxide (MgO), while generally stable, is a basic oxide and could affect the pH balance of local environments if released in large quantities. Item two: a) Assess the product formed. The product formed from the complete combustion of charcoal (carbon) in excess oxygen is carbon dioxide (CO_2). It is a gaseous compound and is classified as a greenhouse gas. b) Advise the friend on the appropriateness of the product formed. The production of carbon dioxide (CO_2) during cooking, especially indoors, is not appropriate without proper ventilation. CO_2 can accumulate in enclosed spaces, displacing oxygen and leading to suffocation. Environmentally, CO_2 is a major greenhouse gas that contributes to global warming. c) Calculate the volume of the gas produced every busy evening. Step 1: Calculate the number of moles of charcoal (carbon) used. The molar mass of carbon (C) is 12 g/mol. Moles of C = Mass of CMolar mass of C = 80.5 g12 g/mol ≈ 6.7083 mol Step 2: Use the mole ratio from the balanced chemical equation to find the moles of carbon dioxide produced. The balanced equation is C_(s) + O_2(g) → CO_2(g). From the equation, 1 mole of C produces 1 mole of CO_2. Moles of CO_2 = Moles of C ≈ 6.7083 mol Step 3: Calculate the volume of carbon dioxide produced, assuming Room Temperature and Pressure (RTP). At RTP, 1 mole of any gas occupies 24 dm^3. Volume of CO_2 = Moles of CO_2 × 24 dm^3/mol Volume of CO_2 = 6.7083 mol × 24 dm^3/mol ≈ 160.9992 dm^3 The volume of carbon dioxide gas produced is approximately 161.0 dm^3. d) Help the friend understand the impact of the product in the environment. Carbon dioxide (CO_2) is a primary greenhouse gas. Its accumulation in the atmosphere traps heat, leading to global warming and climate change. This can result in rising sea levels, extreme weather events, and disruptions to ecosystems. Send me the next one 📸