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Question
Which of the following is not an example of redox reaction?
Options
\[\ce{CuO + H2 -> Cu + H2O}\]
\[\ce{Fe2O3 + 3CO -> 2Fe + 3CO2}\]
\[\ce{2K + F2 -> 2KF}\]
\[\ce{BaCl2 + H2SO4 -> BaSO4 + 2HCl}\]
Solution
\[\ce{BaCl2 + H2SO4 -> BaSO4 + 2HCl}\]
Explanation:
Redox reaction is defined as the simultaneous oxidation and reduction of reacting species. Thus, change in oxidation state will decide whether a reaction is redox or not. Thus, assigning the oxidation states as:
(i) \[\ce{CuO + H2 -> Cu + H2O}\]
Here, oxidation of H and reduction of \[\ce{Cu}\] is taking place.
(ii) \[\ce{Fe2O3 + 3CO -> 2Fe + 3CO2}\]
Here, oxidation of \[\ce{C}\] and reduction of \[\ce{Fe}\] is taking place.
(iii) \[\ce{2K + F2 -> 2KF}\]
Here, the oxidation of \[\ce{K}\] and reduction of \[\ce{F}\] is taking place.
(iv) \[\ce{BaCl2 + H2SO4 -> BaSO4 + 2HCl}\]
This is not a redox reaction, but it is a double displacement reaction.
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