pls explain this....
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Answers
Answer:
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no. 2 is the one that does not show oxidising behaviour
Explanation:
to know if a substance is an oxidizing agent one or all of the following must happen
- it must lose oxygen
- it's oxidation number would reduce
- the substance it's reacting with would be oxidized
- it gains electrons
in the first equation, C is oxidised to CO2 as it gains oxygen and there is an increase in its oxidation number. H2SO4 loses oxygen and is reduced to SO2. this shows that H2SO4 is an oxidising agent
in the second equation, it is basically a double deplacement not a redox reaction. the oxidation number of both compounds remain the same so neither is being oxidised nor reduced.
in the third equation, Cu is oxidized to CuSO4. it's oxidation number increases and it gains oxygen. H2SO4 is also being reduced to SO2 as it oxidation number reduces. so it is an oxidizing agent.
in the last equation, S is oxidises to SO2 and H2SO4 is equally reduced to SO2. S gains oxygen and experiences an increase in oxidation number whereas H2SO4 loses oxygen and experiences a decrease in oxidation number.
Hope it'll help you ....
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