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 when heated, indicated by the mass remaining constant at 10 g and the limewater not turning cloudy. This suggests that no carbon dioxide was produced, and the required temperature for decomposition was likely not achieved.

The reactivity series can predict that the less reactive metals will have their carbonates decompose less easily. Hence, the more reactive a metal is, the more likely its carbonate will decompose or react when heated.

Iron ores must contain enough iron to make extracting the metal economically viable.

The balanced equation for the reduction of iron(III) oxide by carbon is:

$\text{Fe}_2\text{O}_3 + 3\text{C} \rightarrow 2\text{Fe} + 3\text{CO}$

1. Iron from the blast furnace is brittle which limits its applications.
2. Steel is stronger and more ductile, making it more useful for construction and manufacturing.

1. Recycling conserves resources and reduces the need for mining new iron ore.
2. It minimizes pollution and energy use compared to extracting raw materials.
3. It prevents metal corrosion and waste accumulation in landfills, preserving the environment.