Hydrogen-based fuel cells show promise as an alternative fuel source. They use a galvanic cell in which oxygen gas is supplied to one compartment and hydrogen gas to another. The reduction of O2 gas and oxidation of H2 gas are used to generate power. Consider a fuel cell where the cathodic compartment has an O2 partial pressure of 0.21 bar and the anodic compartment has an H2 pressure of 0.4 bar. At room temperature, what is the maximum work produced for every mole of H2 that reacts? What is the value if the fuel cell operates at 650°C? Assume Δhrxn o = constant.