Can someone help me out with this?
Chapter 7: Electrochemistry
148) The first step in producing pure lead from galena (PbS) is as follows:
2 PbS (s) + 3 O2 (g) -> 2 PbO (s) + 2 SO2 (g)
All of the following are true concerning this reaction EXCEPT:
a) Both lead and sulfur are oxidized
b) Oxygen is the oxidizing agent
c) Lead sulfide is the reducing agent
d) Lead is neither oxidized nor reduced
The correct answer is supposed to be A, and I understand why. But I don't understand why D isn't the correct answer. In PbS, S has a -2 charge and Pb has a +2 charge. In PbO, O has a -2 charge and Pb has a +2 charge. The charge doesn't change before or after. Therefore, why can't we say that it's neither oxidized nor reduced?
Chapter 7: Electrochemistry
148) The first step in producing pure lead from galena (PbS) is as follows:
2 PbS (s) + 3 O2 (g) -> 2 PbO (s) + 2 SO2 (g)
All of the following are true concerning this reaction EXCEPT:
a) Both lead and sulfur are oxidized
b) Oxygen is the oxidizing agent
c) Lead sulfide is the reducing agent
d) Lead is neither oxidized nor reduced
The correct answer is supposed to be A, and I understand why. But I don't understand why D isn't the correct answer. In PbS, S has a -2 charge and Pb has a +2 charge. In PbO, O has a -2 charge and Pb has a +2 charge. The charge doesn't change before or after. Therefore, why can't we say that it's neither oxidized nor reduced?
I guess this is what I get for doing questions at the end of a 7-hour study session. Thank you!
