The Reaction:
SnO₂ (s) + 2 H₂ (g) → Sn (s) + 2 H₂O (g)
Explanation:
* Tin(IV) oxide (SnO₂): This is the oxide of tin, where tin has a +4 oxidation state.
* Hydrogen gas (H₂): This is a reducing agent, meaning it donates electrons to other substances.
* Tin (Sn): The tin is reduced from a +4 oxidation state to a 0 oxidation state, forming solid elemental tin.
* Water vapor (H₂O): The hydrogen is oxidized from a 0 oxidation state to a +1 oxidation state, forming water molecules.
Balancing the Equation:
The equation is already balanced, meaning that the number of atoms of each element is the same on both sides.
Key Points:
* This reaction requires heat to proceed.
* The reaction is a classic example of a redox reaction, where one substance is oxidized (loses electrons) while another is reduced (gains electrons).
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