Part II. Non-Spontaneous Redox Reaction Electrolysis of Water: 2 HO 2H(g) + O2(g) Table: Useful reduction half-reactions and their associated potentials. Reaction number Half-reaction Reduction potential 03 + 2H+ + 2e 0 + HO +2.07 || HO + 2H+ + 2e 2HO +1.78 III O + 4H+ + 4e 2HO +1.23 IV O + 2HO + 4e 4OH +0.40 V 2H+ + 2e H 0.00 VI 2HO +2e H + 2 OH- -0.83 Information Statement Remember that the universal indicator is red in the presence of H* and blue in the presence of OH, and the bromothymol blue indicator is yellow in the presence of H* and blue in the presence of OH. Consider the half-cell connected to the negative terminal of the battery: Based on the color of the pH indicator, what ions were produced in this half-cell? 0- O OH- H+ O H Based on the relative amounts of gas in the tube, which gas was produced? H O 0 O SO 3 Identify the half-reaction that occurs at this terminal. VI This half-cell reaction is a(an) oxidation and occurs at the anode