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Questions and Answers
The balanced reaction shows that 4Zn reacts with 16OH- to form 4Zn(OH)42- and NH3.
True
In the half reaction for zinc, Zn reduces to Zn(OH)42- while losing electrons.
False
The conversion of acidic to basic in the reactions involves the addition of H2O molecules to balance the hydrogens.
True
The nitrate ion NO3- gains a total of 8 electrons during the reaction.
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4H2O is added to the equation that includes the nitrate ion to balance the oxygen atoms.
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The combined half reactions lead to a charge balance of 8 negative charges on both sides of the final equation.
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The final equation contains 9 hydroxide ions on the reactants side.
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In the half reaction for zinc, the product formed is Zn(OH)42- along with 2 electrons.
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The equation NO3- + 6H2O + 8e- → NH3 + 9OH- correctly balances all species involved.
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The oxidation state of zinc changes from 0 to +2 in the given reaction.
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Study Notes
Identify ox/red.species
- The reaction is in a basic aqueous solution
- Zn is oxidized
- NO3- is reduced
Balancing the Redox Reaction
- Zinc is oxidized to Zn(OH)42-
- Nitrate is reduced to ammonia
- Balance oxygen by adding water
- Balance hydrogen by adding H+ ions
- Convert the acidic half-reactions to basic conditions by adding OH- ions
- Combine the half-reactions to form a balanced redox reaction
Balancing Half-Reactions
- The half-reaction for the oxidation of zinc: Zn + 4OH- → Zn(OH)42- + 2e-
- The half-reaction for the reduction of nitrate: NO3- + 6H2O + 8e- → NH3 + 9OH-
Balancing the Overall Reaction
- Multiply the zinc half-reaction by 4 to equalize the number of electrons in both half-reactions
- Combine the two half-reactions to get the balanced redox reaction: 4Zn + 7OH- + NO3- + 6H2O → 4Zn(OH)42- + NH3
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Description
Test your knowledge on balancing redox reactions in basic aqueous solutions. The quiz covers the oxidation of zinc and the reduction of nitrate, including the necessary steps to balance half-reactions and the overall reaction. This is essential for understanding redox processes in chemistry.
