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Question
Justify that the following reaction is redox reaction:
\[\ce{2K(s) + F2(g) → 2K+F– (s)}\]
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Solution
The oxidation number of each element in the given reaction can be represented as:
0 0 +1 -1
\[\ce{2K(s) + F2(g) → 2K+F– (s)}\]
In this reaction, the oxidation number of K increases from 0 in K to +1 in KF i.e., K is oxidized to KF. On the other hand, the oxidation number of F decreases from 0 in F2to –1 in KF i.e., F2 is reduced to KF.
Hence, the above reaction is a redox reaction.
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