Consider the unbalanced equation:

Zn(s) + HNO3(aq) → Zn(NO3)2(aq) + N2O(g) + H2O(l)

In the balanced equation, the number of electrons transferred is:

Question

Consider the unbalanced equation:

Zn(s) + HNO3(aq) → Zn(NO3)2(aq) + N2O(g) + H2O(l)

In the balanced equation, the number of electrons transferred is:

BlackTom AI · Accepted Answer

First, restating the problem in my own words: we are balancing a redox equation where zinc metal reacts with nitric acid to form zinc nitrate, nitrogen monoxide oxide (N2O) gas, and water. We are asked for the total number of electrons transferred in the balanced equation.

Option analysis:

Option 8: This corresponds to a total of eight electrons being transferred in the oxidation-reduction process. In the oxidation half-reaction, zinc is oxidized from Zn(0) to Zn2+, which involves loss of 2 electrons per zinc atom. To balance the nitrogen-containing species, nitrogen in HNO3 has oxidation state +5 and ends up in N2O where each nitrogen is in the +1 state. Each N atom thus gains 4 electrons. Since N2O contains two nitrogen atoms, the nitrogen species together gain 2 × 4 = 8 electrons. The overall redox process therefore involves transfer of 8 electrons. This means the balanced equation must involve 4 zinc atoms (to supply 8 electrons total), consistent with typical balancing where Zn coefficient is 4 in front of Zn and 4 Zn atoms supply 8 electrons, while the nitrogen moiety accepts those 8 electrons to become N2O. Hence 8 electrons transferred is correct.

Option 4: If only 4 electrons were transferred in total, that would imply either only two Zn atoms were oxidized or only one N atom changed oxidation state by 4 electrons, which contradicts the stoichiometry needed to produce N2O (two nitrogens in N2O at +1 each from +5 in HNO3) and to balance charge and atoms simultaneously.

Option 6: A total of 6 electrons would require non-integer or inconsistent oxidation state changes for the species involved, or an imbalance in either zinc oxidation or nitrogen reduction that cannot satisfy both mass and charge balance in this reaction.

Option 2: Only 2 electrons transferred would imply a minimal change (e.g., a single Zn atom becoming Zn2+ with a single N changing state by 2 electrons), which does not align with forming N2O (requiring two nitrogens each gaining 4 electrons) and balancing the entire equation. This underestimates the electron bookkeeping required by the reaction.

In summary, the reaction involves four zinc atoms oxidizing to Zn2+ (8 electrons total) and two nitrogen atoms in HNO3 being reduced to form N2O (also accounting for 8 electrons gained by nitrogen). The only option that matches this complete redox balance is 8 electrons transferred.

Chem 1C General Chemis... Self Assessment Quiz 20

Consider the unbalanced equation: Zn(s) + HNO3(aq) → Zn(NO3)2(aq) + N2O(g) + H2O(l) In the balanced equation, the number of electrons transferred is:

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