Question

1. What is the redox state of Oxygen in a molecule of diatomic hydrogen gas (H₂)?

2. NO₂^- + 6e^- -> NH₄⁺ (-0.41 volts) & O₂ + 4e^- -> 2H₂O (+0.82 volts)

If you balance and combine the reactions so that 52 molecules of NH₄⁺ are oxidized to NO₂^-, how many molecules of O₂ will be reduced to H₂O?

3. NO₃^- + 10e^- -> N₂ (E⁰ = +0.74 V) & H⁺ + 2e^- -> H₂ (E⁰ = -0.42 V)

If you balance and combine the reactions so that 225 molecules of H2 gas are oxidized to H⁺, how many molecules of N₂ gas will be produced?

4. 2NO₃^- + 10e^- -> N₂ (+0.74 volts) & 2H⁺ + 2e^- -> H₂ (-0.42 volts)

Using the information given, calculate the ΔE for this reaction, balance the full reaction to determine the n, the number of electrons transfered when 96 molecules of H₂ are oxidized. Finally, use the simplified Nernst Equation to determine the Gibbs Free energy available to do work! ΔG = -nFΔE, where F = 96.48 kJ (mol e^-)

Answer 1