Why does hydrogen give up its electron to a platinum catalyst?

All descriptions of a Hydrogen fueled fuel cell (such as this one) Start with $H_2$ giving up its electrons to a platinum coated anode. Then the $H^+$ ions (protons really) travel through the electrolyte where they find $O_2$ and the $e^-$ they had previously given up at a platinum-coated cathode. At the cathode, these components come together with a sigh of exothermic relief and $H_2O$ drips out.

I have no sense at all what DRIVES the cell. I am guessing that somehow in some context the $H_2$ giving up its electrons to the platinum anode is energetically favorable, but I can't for the life of me think of how pulling electrons away from protons would be favorable.

So what I really want here is to understand what the forces or pseudo-forces are that drive a Fuel Cell. What drives $H_2$ to give up its electrons to the platinum anode?

Any helpful directions to figuring this out would be appreciated.

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Every picture I see does NOT show H or H2 being adsorbed on the platinum anode, but rather the electron from the H going in to the platinum anode and the $H^+$ running away from the platinum so it can diffuse across the membrane and show up at the cathode. –  mwengler Apr 30 '14 at 7:06