(a) Based on standard reduction potentials, would you expect copper metal to oxidize under standard conditions in the presence of oxygen and hydrogen ions? (b) When the Statue of Liberty was refurbished, Teflon spacers were placed between the iron skeleton and the copper metal on the surface of the statue. What role do these spacers play?

(Look up the standard reduction potentials for oxygen, hydrogen, and copper. You can find these in a reference material or online.) For oxygen and hydrogen, the reactions are as follows: \(O_2(g) + 4H^+ + 4e^- \rightarrow 2H_2O(l)\) \(E^{\circ} = 1.23V\) \(2H^+ + 2e^- \rightarrow H_2(g)\) \(E^{\circ} = 0V\) For copper: \(Cu^{2+} + 2e^- \rightarrow Cu(s)\) \(E^{\circ} = 0.34V\) We will use these reduction potentials to determine the feasibility of reactions involving copper and the given substances.

(Based on the reduction potentials, we can now analyze if copper metal would oxidize in the presence of oxygen and hydrogen ions.) If copper metal were to oxidize, the reaction should be: \(Cu(s) \rightarrow Cu^{2+} + 2e^-\) To find the feasibility of this reaction, we need to pair it with another half-reaction involving either oxygen or hydrogen ions. The most favorable pair would be the one with the highest positive value for the overall cell potential (calculated as the difference between the reduction potentials of the two half-reactions). When pairing with oxygen reduction: \(E^{\circ}_{cell} = E^{\circ}_{(O_2/H_2O)} - E^{\circ}_{(Cu^{2+}/Cu)} = 1.23 - 0.34 = 0.89V\) When pairing with hydrogen reduction: \(E^{\circ}_{cell} = E^{\circ}_{(H^+/H_2)} - E^{\circ}_{(Cu^{2+}/Cu)} = 0 - 0.34 = -0.34V\) As per the first pair, the cell's potential is positive (0.89 V), which means the reaction involving copper oxidation and oxygen reduction is feasible.

(Now we can answer Part a of the exercise.) Yes, copper metal would oxidize under standard conditions in the presence of oxygen and hydrogen ions, based on the standard reduction potentials. Specifically, copper will oxidize in the presence of oxygen more so than in the presence of hydrogen ions, as the reaction process has a positive cell potential of 0.89V.

(To answer this question, we need to consider the electrochemical properties of iron and copper.) When two different metals come into contact with each other, galvanic corrosion can occur. Galvanic corrosion is an electrochemical process where one metal corrodes more readily when in electrical contact with a more noble metal. In the case of the Statue of Liberty, the iron skeleton (less noble metal) could corrode in the presence of copper (more noble metal) and the surrounding humid and saline environment.

(Now, let's answer Part b of the exercise referring to the role of Teflon spacers.) Teflon spacers play an essential role in preventing galvanic corrosion between the iron skeleton and the copper surface of the Statue of Liberty. By placing Teflon spacers between the iron and copper, an insulating barrier is created to prevent electrical contact. This barrier protects the iron skeleton from corroding in the presence of the more noble copper metal.