In a redox reaction, the equivalent weight of HNO 2 is found to be 23.5. The reaction products might contain:

Question

In a redox reaction, the equivalent weight of HNO 2 ​ is found to be 23.5. The reaction products might contain:

TestHub · Accepted Answer

Molecular Weight: The molecular weight of HNO₂ is $1 + 14 + (16 \times 2) = 47 g / m o l$ .

n-factor: Since $Eq u i v a l e n t W e i g h t = \frac{M o l ec u l a r W e i g h t}{n - f a c t or}$ , we have $23.5 = \frac{47}{n}$ , which gives $n = 2$ (change in oxidation state).

Initial State: The oxidation state of Nitrogen in HNO₂ is $+ 3$ .

Final States: A change of 2 means the product must have Nitrogen in either the $+ 1$ state (N₂O) or $+ 5$ state (HNO₃).

Conclusion: The correct options are (A) N₂O and (D) HNO₃.

Chemistry - Redox Reactions Question with Solution | TestHub

Options:(select one or more)

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