Which statement is correct about electrons in the balanced half equation for the following (using simplest whole number ratio)? HNO2 → NO3–

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Let's examine the half-reaction provided: HNO2 → NO3–. 
Option a: '2 electrons are produced.' To assess this, determine the oxidation state change for nitrogen, since the nitrogen atom is the element being oxidized. In HNO2 (neutral), let N have oxidation state x. Using x + (+1) + 2(−2) = 0, we get x + 1 − 4 = 0, so x = +3. In NO3–, nitrogen is in the +5 oxidation state (each O is −2, so total for three O is −6; with −1 overall charge, N must be +5 to balance: +5 + (−6) = −1). The change is from +3 to +5, which is a loss of 2 electrons per nitrogen atom. Therefore, the half-reaction involves 2 electrons being produced.

Option b: '2 electrons are required as reactants.' This would imply reduction with two electrons coming in, but in this context nitrogen is being oxidized (increase in oxidation state), so electrons are released, not consumed. Thus this is incorrect.

Option c: '1 electron is produced.' The oxidation state change shows a two-electron transfer, not one. Therefore this is incorrect.

Option d: '1 electron is required as a reactant.' Similar to option b, this mischaracterizes the process; the reaction is an oxidation (electrons produced), not a reduction (electrons required). Hence this is incorrect.

In summary, accounting for the oxidation state change of nitrogen from +3 to +5 yields a two-electron transfer, aligning with an oxidation process that releases electrons in the balanced half-reaction.

MUF0042 Chemistry Unit 2 - Semester 2, 2025 10.13 Quiz: Balancing Redox Reactions

Which statement is correct about electrons in the balanced half equation for the following (using simplest whole number ratio)? HNO2 → NO3–

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