Provide the balanced equation and calculate the value of E° for the formation of O₂ and H₂O from H₂O₂ given the following half-reactions and corresponding E° values:
H₂O₂(aq) + 2 H⁺(aq) + 2e⁻ → 2 H₂O(l)                E°_H2O2→H2O = 1.78 V
O₂(g) + 2 H⁺(aq) + 2e⁻ → H₂O₂(aq)                     E°_O2→H2O2 = 0.70 V
Determine if the reaction is spontaneous under standard-state conditions.

• A. 2H₂O₂(aq) → 2H₂O(l) + O₂(g)
  E°_cell = −1.08 V
  The reaction is nonspontaneous under standard-state conditions.
• B. 3H₂O₂(aq) + 2H⁺(aq)→ 4H₂O(l) + O₂(g)
  E°_cell = 2.48 V
  The reaction is spontaneous under standard-state conditions.
• C. 2H₂O₂(aq) → 2H₂O(l) + O₂(g)
  E°_cell = 1.08 V
  The reaction is spontaneous under standard-state conditions.
• D. 3H₂O₂(aq) + 2H⁺(aq)→ 4H₂O(l) + O₂(g)
  E°_cell = −2.48 V
  The reaction is spontaneous under standard-state conditions.

Answer: (C)