In a reaction, 3 moles of electrons are gained by 1 mole of HNO3. Assuming no change in O.N. of hydrogen and 23 oxygen, the possible product obtained due to reduction will be :
Correct answer: C. 1 mole of NO
- A. 1 mole of NO2
- B. 0.5 mole of N2O
- C. 1 mole of NO
- D. 0.5 mole of N2O3
Explanation
In this reaction, the reduction of HNO3 involves a change in the oxidation state of nitrogen from +5 to +2, which corresponds to the formation of NO. The balanced reduction equation supports the production of 1 mole of NO when 3 moles of electrons are gained. Other options such as NO2 and N2O3 do not match the stoichiometry of the electron transfer, while N2O involves a different oxidation state change that does not align with the electron gain described.
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Electrochemistry describes electron transfer through oxidation and reduction, identifies oxidizing and reducing agents, and applies oxidation numbers to balance redox equations. It also covers electrode potential and the standard hydrogen electrode, which provides the reference for comparing the reduction tendencies of other electrodes.
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