(b) Using the standard reduction potentials in Appendix E, calculate the standard voltage generated by the hydrogen fuel cell in acidic solution.

Verified step by step guidance

1. Identify the half-reactions involved in the hydrogen fuel cell. In an acidic solution, the reactions are: the oxidation of hydrogen (H₂) and the reduction of oxygen (O₂).
2. Write the half-reactions: Oxidation half-reaction: H₂ → 2H⁺ + 2e⁻. Reduction half-reaction: O₂ + 4H⁺ + 4e⁻ → 2H₂O.
3. Look up the standard reduction potentials (E°) for each half-reaction in Appendix E. Note that the standard reduction potential for the oxidation reaction will be the negative of the value listed, as it is written as a reduction.
4. Calculate the standard cell potential (E°cell) using the formula: E°cell = E°(cathode) - E°(anode). Substitute the values from the standard reduction potentials you found.
5. Ensure that the overall cell reaction is balanced in terms of both mass and charge, and verify that the calculated E°cell is positive, indicating a spontaneous reaction under standard conditions.