Metals are extracted from ores in the Earth’s crust - AQA - GCSE Chemistry - Question 3 - 2016 - Paper 1

The solid product formed when copper carbonate is heated is copper oxide.

The potassium carbonate did not decompose or change when heated. This is indicative that the temperature might not have been sufficiently high to induce any reaction. Furthermore, the mass of the potassium carbonate remained constant, and the limewater did not turn cloudy, showing that no carbon dioxide was produced.

The reactivity series ranks metals based on their reactivity. A more reactive metal will have its carbonate decompose more easily upon heating, while less reactive metals may require higher temperatures or might not decompose at all. Thus, to predict which metal carbonate reacts most easily, one would look for the carbonate associated with the most reactive metal.

Iron ores must contain enough iron to be economically viable for extraction.

The balanced equation for the reaction is:

1. Steel is stronger and more flexible than iron, making it more suitable for construction and manufacturing.
2. Steel has specific properties, such as improved resistance to rust compared to raw iron, which enhances its durability.

1. Recycling conserves resources and reduces the need to extract additional iron ore, minimizing environmental impact.
2. Reusing metal components can be less efficient and may compromise safety or quality.
3. Landfills have limited space, and diverting steel from them helps reduce land pollution and conserves land resources.