Question

Fluorine reacts with ice and results in the change:
\(H_2O(s) + F_2{(g)} \rightarrow HF{(g)} + HOF{(g)}\) Justify that this reaction is a redox reaction.

Answer 1

Given reaction:

H₂O(s) + F₂(g) → HF(g) + HOF(g)

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Justification that the reaction is a redox reaction:

To justify whether a reaction is a redox reaction, we examine the changes in oxidation states of the elements involved.

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Oxidation states of elements:

Before reaction:

• In H₂O: Hydrogen = +1, Oxygen = −2
• In F₂: Fluorine = 0 (elemental state)

After reaction:

• In HF: Hydrogen = +1, Fluorine = −1
• In HOF: Hydrogen = +1, Oxygen = 0, Fluorine = −1

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Changes in oxidation states:

• Fluorine changes from 0 in F₂ to −1 in HF and HOF. This shows reduction.
• Oxygen changes from −2 in H₂O to 0 in HOF. This shows oxidation.

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Conclusion:

Since fluorine undergoes reduction and oxygen undergoes oxidation simultaneously, the reaction involves both oxidation and reduction.

Therefore, the given reaction is a redox reaction.