For #11 choice E is correct b/c the E0 for the rxn shown is a big negative number and as u know the more positive an E0 is the better its ability to oxidize hence a better oxidizing agent, so in our case the E0=-2.174 thus its a good reducing agent which again means that it readily oxidizes. you can think of X(s) as an element like Li(s) which really wants to get rid of one electron and become oxidized.

1.6 would be the Cell Voltage. The question asked for the equilibrium constant. That would be found using the Nerst equation, which I believe is not necessary for the DAT. Google it if you wish.

For 2. the negative E0 means that it is nonspontaneous. This is the reduction and therefore X+ is poorly reduced. However, any nonspontaneous reaction becomes spontaneous when you flip it. So flipping the reaction we see that X is oxidized spontaneously.

For #11 choice E is correct b/c the E0 for the rxn shown is a big negative number and as u know the more positive an E0 is the better its ability to oxidize hence a better oxidizing agent, so in our case the E0=-2.174 thus its a good reducing agent which again means that it readily oxidizes. you can think of X(s) as an element like Li(s) which really wants to get rid of one electron and become oxidized.

A negative Eo does not mean that it is being oxidized. There can be a negative Eo when a reduction is spontaneous also. Here, since the the reduction half reaction happens to have a negative Eo, we know that the oxidation would have a positive, and would hence be spontaneous.